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engineering
the science and engineering of materials

Chemistry 10th Edition Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste - Solutions

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.a. 0.0200 mole of sodium phosphate in 10.0 mL of solution b. 0.300 mole of barium nitrate in 600.0 mL of solutionc. 1.00 g of potassium chloride in 0.500 L of solutiond. 132 g of
Which of the following solutions of strong electrolytes contains the largest number of ions: 100.0 mL of 0.100 M NaOH, 50.0 mL of 0.200 M BaCl2, or 75.0 mL of 0.150 M Na3PO4?
What mass of NaOH is contained in 250.0 mL of a 0.400 M sodium hydroxide solution?
If 10. g of AgNO3 is available, what volume of 0.25 M AgNO3 solution can be prepared?
The sodium level in a patient’s blood was measured at 137 mmol/L. If 15.0 mL of blood is drawn from this patient, what mass of sodium would be present?
High-density lipoprotein (HDL) cholesterol is the “good” cholesterol because adequate levels reduce the risk of heart disease and stroke. HDL levels between 40. and 59 mg/dL are typical for a healthy individual. What is this range of HDL cholesterol in units of mol/L? The formula for
Describe how you would prepare 2.00 L of each of the following solutions.a. 0.250 M NaOH from solid NaOHb. 0.250 M NaOH from 1.00 M NaOH stock solutionc. 0.100 M K2CrO4 from solid K2CrO4d. 0.100 M K2CrO4 from 1.75 M K2CrO4 stock solution
A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.00-mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.
A solution was prepared by mixing 50.00 mL of 0.100 M HNO3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.
Suppose 50.0 mL of 0.250 M CoCl2 solution is added to 25.0 mL of 0.350 M NiCl2 solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive.
When the following solutions are mixed together, what precipitate (if any) will form?a. FeSO4(aq) + KCl(aq)b. Al(NO3)3(aq) + Ba(OH)2(aq)c. CaCl2(aq) + Na2SO4(aq)d. K2S(aq) + Ni(NO3)2(aq)
Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na2SO4 is added. Which cations could be present in the unknown soluble ionic compound?
What mass of Na2CrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100-M solution of AgNO3?
What mass of iron(III) hydroxide precipitate can be produced by reacting 75.0 mL of 0.105 M iron(III) nitrate with 125 mL of 0.150 M sodium hydroxide?
What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride is mixed with 100.0 mL of a 0.100-M solution of iron(III) sulfate?
The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potassium hydroxide.a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation
A 1.42-g sample of a pure compound, with formula M2SO4, was dissolved in water and treated with an excess of aqueous calcium chloride, resulting in the precipitation of all the sulfate ions as calcium sulfate. The precipitate was collected, dried, and found to weigh 1.36 g. Determine the atomic
Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions. a. HCIO4 (aq) + Mg(OH)₂(s) → b. HCN(aq) + NaOH(aq) C. HCl(aq) + NaOH(aq)
Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions. a. HNO3(aq) + Al(OH)3(s) → b. HC₂H₂O₂(aq) + KOH(aq) → C. Ca(OH)₂(aq) + HCl(aq) →
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.a. If you had an
What acid and what base would react in aqueous solution so that the following salts appear as products in the formula equation? Write the balanced formula equation for each reaction.a. Potassium perchlorateb. Cesium nitratec. Calcium iodide
A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?
Specify which of the following are oxidation–reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. 2+ a. Cu(s) + 2Ag+ (aq) →2Ag(s) + Cu²+ (aq) b. HCl(g) + NH3(g) →NH4Cl(s) c. SiC¹4(1) + 2H₂O(l) →4HCl(aq)
A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.
Balance the following oxidation–reduction reactions that occur in acidic solution using the half-reaction method. a. Cu(s) + NO3(aq) → Cu²+ (aq) + NO(g) b. Cr₂O72 (aq) + Cl¯(aq) → Cr³+ (aq) + Cl₂(g) c. Pb(s) + PbO₂ (s) + H₂SO4(aq) → PbSO4(s) d. Mn²+ (aq) + NaBiO3(s)
Specify which of the following equations represent oxidation– reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced. a. CH4(g) + H₂O(g) →CO(g) + 3H₂(g) b. 2AgNO3(aq) + Cu(s) → Cu(NO3)₂(aq) + 2Ag(s) c.
Balance the following oxidation–reduction reactions that occur in basic solution. a. Cr(s) + CrO2 (aq) → Cr(OH)3(s) b. MnO4 (aq) + S²(aq) →MnS (s) + S(s) c. CN (aq) + MnO4 (aq) →CNO (aq) + MnO₂ (s)
Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction isBalance this equation. NaCl(aq) + H₂SO4 (aq) + MnO₂ (s) Na₂SO4 (aq) + MnCl₂(aq) + H₂O(1) + Cl₂(g)
A solution of permanganate is standardized by titration with oxalic acid (H2C2O4). It required 28.97 mL of the permanganate solution to react completely with 0.1058 g of oxalic acid. The unbalanced equation for the reaction isWhat is the molarity of the permanganate solution? MnO4 (aq) +
The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe2+ ions. This solution is then titrated with KMnO4 solution, producing Fe3+ and Mn2+ ions in acidic solution. If it required 38.37 mL of
You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy
The figures below are molecular-level representations of four aqueous solutions of the same solute. Arrange the solutions from most to least concentrated. Solution A (1.0 L) Solution C (2.0 L) Solution B (4.0 L) Solution D (2.0 L)
An average human being has about 5.0 L of blood in his or her body. If an average person were to eat 32.0 g of sugar (sucrose, C12H22O11, 342.30 g/mol), and all that sugar were dissolved into the bloodstream, how would the molarity of the blood sugar change?
A 230.-mL sample of a 0.275-M CaCl2 solution is left on a hot plate overnight; the following morning, the solution is 1.10 M. What volume of water evaporated from the 0.275 M CaCl2 solution?
Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.06 g of precipitate. Determine the concentration of the NaOH solution.
Some of the substances commonly used in stomach antacids are MgO, Mg(OH)2, and Al(OH)3.a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances.b. Which of these substances will neutralize the greatest amount of 0.10 M HCl per gram?
Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g sample of a medication containing the drug was treated to destroy the organic material and to release all the chlorine as chloride ion. When the filtered solution containing chloride ion was treated
Douglasite is a mineral with the formula 2KCl # FeCl2 # 2H2O. Calculate the mass percent of douglasite in a 455.0-mg sample if it took 37.20 mL of a 0.1000-M AgNO3 solution to precipitate all the Cl- as AgCl. Assume the douglasite is the only source of chloride ion.
Saccharin (C7H5NO3S) is sometimes dispensed in tablet form. Ten tablets with a total mass of 0.5894 g were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of BaSO4 obtained was
One of the classic methods for determining the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas.
Calculate the concentration of all ions present when 0.160 g of MgCl2 is dissolved in 100.0 mL of solution.
A solution is prepared by dissolving 0.6706 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the oxalic acid solution?
For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate will form. Sr(NO3)₂(aq) + K3PO4(aq) →→→→ K₂CO3(aq) + AgNO3(aq) →→→→→→→ NaCl(aq) + KNO3(aq) KCl(aq) +
A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?
The zinc in a 1.343-g sample of a foot powder was precipitated as ZnNH4PO4. Strong heating of the precipitate yielded 0.4089 g Zn2P2O7. Calculate the mass percent of zinc in the sample of foot powder.
A 50.00-mL sample of aqueous Ca(OH)2 requires 34.66 mL of a 0.944-M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.
In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution?
Complete and balance each acid–base reaction. a. H₂PO4(aq) + NaOH(aq) → Contains three acidic hydrogens b. H₂SO4(aq) + Al(OH)3(s) → Contains two acidic hydrogens c. H₂Se(aq) + Ba(OH)₂(aq) → Contains two acidic hydrogens d. H₂C₂O4(aq) + NaOH(aq) → Contains two acidic
You made 100.0 mL of a lead(II) nitrate solution for lab but forgot to cap it. The next lab session you noticed that there was only 80.0 mL left (the rest had evaporated). In addition, you forgot the initial concentration of the solution. You decide to take 2.00 mL of the solution and add an excess
A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.
It took 25.06 ±0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 83). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass.
You have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246% nitrogen by mass. The ionic compound in solution B consists of potassium, chromium, and oxygen; chromium has an oxidation state of +6 and there are 2 potassiums and 1 chromium in the formula. The
You pass a road sign saying “New York 112 km.” If you drive at a constant speed of 65 mi/h, how long should it take you to reach New York? If your car gets 28 miles to the gallon, how many liters of gasoline are necessary to travel 112 km?
In recent years, there has been a large push for an increase in the use of renewable resources to produce the energy we need to power our vehicles. One of the newer fuels that has become more widely available is E85, a mixture of 85% ethanol and 15% gasoline. Despite being more environmentally
Convert the following Fahrenheit temperatures to the Celsius and Kelvin scales.a. -459οF, an extremely low temperatureb. -40.οF, the answer to a trivia questionc. 68οF, room temperatured. 7 × 107 οF, temperature required to initiate fusion reactions in the sun
Use the figure below to answer the following questions. a. Derive the relationship between οC and οX.b. If the temperature outside is 22.0οC, what is the temperature in units of οX?c. Convert 58.0οX to units of οC, K, and οF. 130°C -10°C 50°X 0°X
The average daytime temperatures on the earth and Jupiter are 72οF and 313 K, respectively. Calculate the difference in temperature, in οC, between these two planets.
A material will float on the surface of a liquid if the material has a density less than that of the liquid. Given that the density of water is approximately 1.0 g/mL, will a block of material having a volume of 1.2 × 104 in3 and weighing 350 lb float or sink when placed in a reservoir of water?
One metal object is a cube with edges of 3.00 cm and a mass of 140.4 g. A second metal object is a sphere with a radius of 1.42 cm and a mass of 61.6 g. Are these objects made of the same or different metals? Assume the calculated densities are accurate to ±1.00%.
A star is estimated to have a mass of 2 × 1036 kg. Assuming it to be a sphere of average radius 7.0 × 105 km, calculate the average density of the star in units of grams per cubic centimeter.
A rectangular block has dimensions 2.9 cm × 3.5 cm × 10.0 cm. The mass of the block is 615.0 g. What are the volume and density of the block?
Diamonds are measured in carats, and 1 carat = 0.200 g. The density of diamond is 3.51 g/cm3.a. What is the volume of a 5.0-carat diamond?b. What is the mass in carats of a diamond measuring 2.8 mL?
At room temperature the element bromine, Br2, is a liquid with a density of 3.12 g/cm3 . Calculate the mass of 125 mL of bromine. What volume does 85.0 g of bromine occupy?
A sample containing 33.42 g of metal pellets is poured into a graduated cylinder initially containing 12.7 mL of water, causing the water level in the cylinder to rise to 21.6 mL. Calculate the density of the metal.
The density of pure silver is 10.5 g/cm3 at 20οC. If 5.25 g of pure silver pellets is added to a graduated cylinder containing 11.2 mL of water, to what volume level will the water in the cylinder rise?
In each of the following pairs, which has the greater volume?a. 1.0 kg of feathers or 1.0 kg of leadb. 100 g of gold or 100 g of waterc. 1.0 L of copper or 1.0 L of mercury
Match each description below with the following microscopic pictures. More than one picture may fit each description. A picture may be used more than once or not used at all.a. A gaseous compoundb. A mixture of two gaseous elementsc. A solid elementd. A mixture of a gaseous element and a gaseous
A copper wire (density = 8.96 g/cm3 ) has a diameter of 0.25 mm. If a sample of this copper wire has a mass of 22 g, how long is the wire?
Define the following terms: solid, liquid, gas, pure substance, element, compound, homogeneous mixture, heterogeneous mixture, solution, chemical change, physical change.
Suppose a teaspoon of magnesium filings and a teaspoon of powdered sulfur are placed together in a metal beaker. Would this constitute a mixture or a pure substance? Suppose the magnesium filings and sulfur are heated so that they react with each other, forming magnesium sulfide. Would this still
If a piece of hard, white blackboard chalk is heated strongly in a flame, the mass of the piece of chalk will decrease, and eventually the chalk will crumble into a fine white dust. Does this change suggest that the chalk is composed of an element or a compound?
During a very cold winter, the temperature may remain below freezing for extended periods. However, fallen snow can still disappear, even though it cannot melt. This is possible because a solid can vaporize directly, without passing through the liquid state. Is this process (sublimation) a physical
Classify the following as physical or chemical changes.a. Moth balls gradually vaporize in a closet.b. Hydrofluoric acid attacks glass and is used to etch calibration marks on glass laboratory utensils.c. A French chef making a sauce with brandy is able to boil off the alcohol from the brandy,
The properties of a mixture are typically averages of the properties of its components. The properties of a compound may differ dramatically from the properties of the elements that combine to produce the compound. For each process described below, state whether the material being discussed is most
Two spherical objects have the same mass. One floats on water; the other sinks. Which object has the greater diameter? Explain.
A 194-g sample of caffeine (C8H10N4O2) contains 6.02 × 1023 molecules of caffeine. If a typical 10-hour energy drink contains 422 mg of caffeine, how many molecules of caffeine are present in the drink?
The active ingredient of aspirin tablets is acetylsalicylic acid, which has a density of 1.4 g/cm3. In a lab class, a student used paper chromatography to isolate another common ingredient of headache remedies. The isolated sample had a mass of 0.384 g and a volume of 0.32 cm3. Given the data in
Lipitor, a pharmaceutical drug that has been shown to lower “bad” cholesterol levels while raising “good” cholesterol levels in patients taking the drug, had over $3 billion in sales in 2015. Assuming one 2.5-g pill contains 4.0% of the active ingredient by mass, what mass in kg of active
The contents of one 40. lb bag of topsoil will cover 10. square feet of ground to a depth of 1.0 inch. What number of bags is needed to cover a plot that measures 200. by 300. m to a depth of 4.0 cm?
A parsec is an astronomical unit of distance where 1 parsec = 3.26 light years (1 light year equals the distance traveled by light in one year). If the speed of light is 186,000 mi/s, calculate the distance in meters of an object that travels 9.6 parsecs.
A person with high cholesterol has 250 mg of cholesterol per 100.0 mL of blood. If the total blood volume of the person is 5.4 L, what is the total mass (in grams) of cholesterol present in the person’s blood?
A column of liquid is found to expand linearly on heating. Assume the column rises 5.25 cm for a 10.0οF rise in temperature. If the initial temperature of the liquid is 98.6οF, what will the final temperature be in οC if the liquid has expanded by 18.5 cm?
The longest river in the world is the Nile River with a length of 4145 mi. How long is the Nile in cable lengths, meters, and nautical miles?Use these exact conversions to help solve the problem: 6 ft 1 fathom = = 100 fathoms = 1 cable length 10 cable lengths = 1 nautical mile 3 nautical miles = 1
According to the Official Rules of Baseball, a baseball must have a circumference not more than 9.25 in or less than 9.00 in and a mass not more than 5.25 oz or less than 5.00 oz. What range of densities can a baseball be expected to have? Express this range as a single number with an accompanying
Which of the following statements is(are) true?a. A spoonful of sugar is a mixture.b. Only elements are pure substances.c. Air is a mixture of gases.d. Gasoline is a pure substance.e. Compounds can be broken down only by chemical means.
Which of the following describes a chemical property?a. The density of iron is 7.87 g/cm3 .b. A platinum wire glows red when heated.c. An iron bar rusts.d. Aluminum is a silver-colored metal.
A rule of thumb in designing experiments is to avoid using a result that is the small difference between two large measured quantities. In terms of uncertainties in measurement, why is this good advice?
On October 21, 1982, the Bureau of the Mint changed the composition of pennies (see Exercise 120). Instead of an alloy of 95% Cu and 5% Zn by mass, a core of 99.2% Zn and 0.8% Cu with a thin shell of copper was adopted. The overall composition of the new penny was 97.6% Zn and 2.4% Cu by mass. Does
Which of the following is true about an individual atom? Explain.a. An individual atom should be considered to be a solid.b. An individual atom should be considered to be a liquid.c. An individual atom should be considered to be a gas.
Heat is applied to an ice cube in a closed container until only steam is present. Draw a representation of this process, assuming you can see it at an extremely high level of magnification. What happens to the size of the molecules? What happens to the total mass of the sample?
Distinguish between the terms family and period in connection with the periodic table. For which of these terms is the term group also used?
When metals react with nonmetals, an ionic compound generally results. What is the predicted general formula for the compound formed between an alkali metal and sulfur? Between an alkaline earth metal and nitrogen? Between aluminum and a halogen?
Why is the term “sodium chloride molecule” incorrect whereas the term “carbon dioxide molecule” is correct?
Why do we call Ba(NO3)2 barium nitrate, but we call Fe(NO3)2 iron(II) nitrate?
Why is calcium dichloride not the correct systematic name for CaCl2?
The common name for NH3 is ammonia. What would be the systematic name for NH3? Support your answer.
What refinements had to be made in Dalton’s atomic theory to account for Gay-Lussac’s results on the combining volumes of gases?
When hydrogen is burned in oxygen to form water, the composition of water formed does not depend on the amount of oxygen reacted. Interpret this in terms of the law of definite proportion.
The two most reactive families of elements are the halogens and the alkali metals. How do they differ in their reactivities?

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