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chemistry
physical chemistry
Questions and Answers of
Physical Chemistry
Give an example of a polyprotic acid and write equations for the successive neutralizations of the acidic hydrogen atoms of the acid molecule to produce a series of salts.
Decide whether a reaction occurs for each of the following. If it does not, write NR after the arrow. If it does, write the balanced molecular equation; then write the net ionic equation. a. Al(OH)3
Complete and balance each of the following molecular equations, including phase labels, if a reaction occurs. Then write the net ionic equation. If no reaction occurs, write NR after the arrow. a.
Complete and balance each of the following molecular equations, including phase labels, if a reaction occurs. Then write the net ionic equation. If no reaction occurs, write NR after the arrow. a.
Describe in words how you would do each of the following preparations. Then give the molecular equation for each preparation. a. CuCl2(s) from CuSO4(s) b. Ca(C2H3O2)2(s) from CaCO3(s) c. NaNO3(s)
Describe in words how you would do each of the following preparations. Then give the molecular equation for each preparation. a. MgCl2(s) from MgCO3(s) b. NaNO3(s) from NaCl(s) c. Al(OH)3(s) from
Classify each of the following reactions as a combination reaction, decomposition reaction, displacement reaction, or combustion reaction. a. When they are heated, ammonium dichromate crystals,
Classify each of the following reactions as a combination reaction, decomposition reaction, displacement reaction, or combustion reaction. a. When solid calcium oxide, CaO, is exposed to gaseous
Consider the reaction of all pairs of the following compounds in water solution: Ba(OH)2, Pb(NO3)2, H2SO4, NaNO3, MgSO4. a. Which pair (or pairs) forms one insoluble compound and one soluble compound
Consider the reaction of all pairs of the following compounds in water solution: Sr(OH)2, AgNO3, H3PO4, KNO3, CuSO4. a. Which pair (or pairs) forms one insoluble compound and one soluble compound
An aqueous solution contains 4.50 g of calcium chloride, CaCl2, per liter. What is the molarity of CaCl2? When calcium chloride dissolves in water, the calcium ions, Ca2+, and chloride ions, Cl, in
An aqueous solution contains 3.45 g of iron(III) sulfate, Fe2(SO4)3, per liter. What is the molarity of Fe2(SO4)3? When the compound dissolves in water, the Fe3 ions and SO42 ions in the crystal go
A stock solution of potassium dichromate, K2Cr2O7, is made by dissolving 89.3 g of the compound in 1.00 L of solution. How many milliliters of this solution are required to prepare 1.00 L of 0.100 M
A 71.2-g sample of oxalic acid, H2C2O4, was dissolved in 1.00 L of solution. How would you prepare 1.00 L of 0.150 M H2C2O4 from this solution?
A solution contains 6.00% (by mass) NaBr (sodium bromide). The density of the solution is 1.046 g/cm3. What is the molarity of NaBr?
An aqueous solution contains 4.00% NH3 (ammonia) by mass. The density of the aqueous ammonia is 0.979 g/mL. What is the molarity of NH3 in the solution?
A barium mineral was dissolved in hydrochloric acid to give a solution of barium ion. An excess of potassium sulfate was added to 50.0 mL of the solution, and 1.128 g of barium sulfate precipitate
Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCl2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was
You have a sample of a rat poison whose active ingredient is thallium(I) sulfate. You analyze this sample for the mass percentage of active ingredient by adding potassium iodide to precipitate yellow
An antacid tablet has calcium carbonate as the active ingredient; other ingredients include a starch binder. You dissolve the tablet in hydrochloric acid and filter off insoluble material. You add
A sample of CuSO4 ∙ 5H2O was heated to 110oC, where it lost water and gave another hydrate of copper(II) ion that contains 32.50% Cu. A 98.77-mg sample of this new hydrate gave 116.66 mg of barium
Give an example of a displacement reaction. What is the oxidizing agent? What is the reducing agent?
A sample of CuSO4 ∙ 5H2O was heated to 100oC, where it lost water and gave another hydrate of copper(II) ion that contained 29.76% Cu. An 85.42-mg sample of this new hydrate gave 93.33 mg of barium
A water-soluble compound of gold and chlorine is treated with silver nitrate to convert the chlorine completely to silver chloride, AgCl. In an experiment, 328 mg of the compound gave 464 mg of
A solution of scandium chloride was treated with silver nitrate. The chlorine in the scandium compound was converted to silver chloride, AgCl. A 58.9-mg sample of scandium chloride gave 167.4 mg of
A 0.608-g sample of fertilizer contained nitrogen as ammonium sulfate, (NH4)2SO4. It was analyzed for nitrogen by heating with sodium hydroxide. (NH4)2SO4(s) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l ) +
An antacid tablet contains sodium hydrogen carbonate, NaHCO3, and inert ingredients. A 0.500-g sample of powdered tablet was mixed with 50.0 mL of 0.190 M HCl (hydrochloric acid). The mixture was
You order a glass of juice in a restaurant, only to discover that it is warm and too sweet. The sugar concentration of the juice is 3.47 M, but you would like it reduced to a concentration of 1.78 M.
If 45.1 mL of a solution containing 8.30 g of silver nitrate is added to 30.6 mL of 0.511 M sodium carbonate solution, calculate the molarity of silver ion in the resulting solution. (Assume volumes
If 38.2 mL of 0.248 M aluminum sulfate solution is diluted with deionized water to a total volume of 0.639 L, how many grams of aluminum ion are present in the diluted solution?
An aluminum nitrate solution is labeled 0.256 M. If 31.6 mL of this solution is diluted to a total of 63.7 mL, calculate the molarity of nitrate ion in the resulting solution.
Zinc acetate is sometimes prescribed by physicians for the treatment of Wilson’s disease, which is a genetically caused condition wherein copper accumulates to toxic levels in the body. If you were
Arsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent insect damage. Arsenic acid has three acidic protons. Say you take a 26.14-mL sample of arsenic acid
When the following equation is balanced by the halfreaction method using the smallest set of whole-number stoichiometric coefficients possible, how many electrons are canceled when the two
Identify each of the following reactions as being a neutralization, precipitation, or oxidation–reduction reaction. a. Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) b. Na2SO4(aq) + Hg(NO3)2(aq) →
A 414-mL sample of 0.196 MMgBr2 solution is prepared in a large flask. A 43.0-mL portion of the solution is then placed into an empty 100.0-mL beaker. What is the concentration of the solution in the
Three 1.0-g samples of PbCl2, KCl, and CaCl2 are placed in separate 500-mL beakers. In each case, enough 25oC water is added to bring the total volume of the mixture to 250 mL. Each of the mixtures
Lead(II) nitrate reacts with cesium sulfate in an aqueous precipitation reaction. What are the formulas of lead(II) nitrate and cesium sulfate? Write the molecular equation and net ionic equation for
Silver nitrate reacts with strontium chloride in an aqueous precipitation reaction. What are the formulas of silver nitrate and strontium chloride? Write the molecular equation and net ionic equation
Elemental bromine is the source of bromine compounds. The element is produced from certain brine solutions that occur naturally. These brines are essentially solutions of calcium bromide that, when
Barium carbonate is the source of barium compounds. It is produced in an aqueous precipitation reaction from barium sulfide and sodium carbonate. (Barium sulfide is a soluble compound obtained by
Mercury(II) nitrate is treated with hydrogen sulfide, H2S, forming a precipitate and a solution. Write the molecular equation and the net ionic equation for the reaction. An acid is formed; is it
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
Mercury(II) nitrate is treated with hydrogen sulfide, H2S, forming a precipitate and a solution. Write the molecular equation and the net ionic equation for the reaction. An acid is formed; is it
Iron forms a sulfide with the approximate formula Fe7S8. Assume that the oxidation state of sulfur is –2 and that iron atoms exist in both +2 and +3 oxidation states. What is the ratio of Fe(II)
A transition metal X forms an oxide of formula X2O3. It is found that only 50% of X atoms in this compound are in the +3 oxidation state. The only other stable oxidation states of X are +2 and +5.
What volume of a solution of ethanol, C2H6O, that is 94.0% ethanol by mass contains 0.200 mol C2H6O? The density of the solution is 0.807 g/mL.
What volume of a solution of ethylene glycol, C2H6O2, that is 56.0% ethylene glycol by mass contains 0.350 mol C2H6O2? The density of the solution is 1.072 g/mL.
A 10.0-mL sample of potassium iodide solution was analyzed by adding an excess of silver nitrate solution to produce silver iodide crystals, which were filtered from the solution. KI(aq) + AgNO3(aq)
A 25.0-mL sample of sodium sulfate solution was analyzed by adding an excess of barium chloride solution to produce barium sulfate crystals, which were filtered from the solution. Na2SO4(aq) +
A metal, M, was converted to the sulfate,M2(SO4)3. Then a solution of the sulfate was treated with barium chloride to give barium sulfate crystals, which were filtered off. M2(SO4)3(aq) + 3BaCl2(aq)
A metal, M, was converted to the chloride, MCl2. Then a solution of the chloride was treated with silver nitrate to give silver chloride crystals, which were filtered from the solution. MCl2(aq) +
Phosphoric acid is prepared by dissolving phosphorus(V) oxide, P4O10, in water. What is the balanced equation for this reaction? How many grams of P4O10 are required to make 1.50 L of aqueous
Iron(III) chloride can be prepared by reacting iron metal with chlorine. What is the balanced equation for this reaction? How many grams of iron are required to make 3.00 L of aqueous solution
An alloy of aluminum and magnesium was treated with sodium hydroxide solution, in which only aluminum reacts. 2Al(s) + 2NaOH(aq) + 6H2O(l ) → 2NaAl(OH)4(aq) + 3H2(g) If a sample of alloy weighing
An alloy of iron and carbon was treated with sulfuric acid, in which only iron reacts. 2Fe(s) + 3H2SO4(aq) → Fe2(SO4)3(aq) + 3H2(g) If a sample of alloy weighing 2.358 g gave 0.1152 g of hydrogen,
Determine the volume of sulfuric acid solution needed to prepare 37.4 g of aluminum sulfate, Al2(SO4)3, by the reaction 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) → 3H2(g) The sulfuric acid solution,
Determine the volume of sodium hydroxide solution needed to prepare 26.2 g sodium phosphate, Na3PO4, by the reaction 3NaOH(aq) + H3PO4(aq) → Na3PO4(aq) + 3H2O(l) The sodium hydroxide solution,
The active ingredients of an antacid tablet contained only magnesium hydroxide and aluminum hydroxide. Complete neutralization of a sample of the active ingredients required 48.5 mL of 0.187 M
The active ingredients in an antacid tablet contained only calcium carbonate and magnesium carbonate. Complete reaction of a sample of the active ingredients required 41.33 mL of 0.08750 M
Part 1
Define the terms strong electrolyte and weak electrolyte. Give an example of each.
Part 1 a. Both NaCl and MgCl2 are soluble ionic compounds. Write the balanced chemical equations for these two substances dissolving in water.
You need to perform gravimetric analysis of a water sample in order to determine the amount of Ag+ present.
In this problem you need to draw two pictures of solutions in beakers at different points in time. Time zero (t = 0) will be the hypothetical instant at which the reactants dissolve in the solution
You come across a beaker that contains water, aqueous ammonium acetate, and a precipitate of calcium phosphate.
Equal quantities of the hypothetical strong acid HX, weak acid HA, and weak base BZ, are added to separate beakers of water, producing the solutions depicted in the drawings. In the drawings, the
Try and answer the following questions without using a calculator.
If one mole of the following compounds were each placed into separate beakers containing the same amount of water, rank the Cl(aq) concentrations from highest to lowest (some may be equivalent):
Using solubility rules, predict the solubility in water of the following ionic compounds. a. PbS b. AgNO3 c. Na2CO3 d. CaI2
Explain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound.
Using solubility rules, predict the solubility in water of the following ionic compounds. a. Al(OH)3 b. Li3P c. NH4Cl d. NaOH
Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, indicate what ions you would expect to be present in solution. a. AgBr b.
Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, indicate what ions you would expect to be present in solution. a.
Write net ionic equations for the following molecular equations. HBr is a strong electrolyte. a. HBr(aq) + KOH(aq) → KBr(aq) + H2O(l) b. AgNO3(aq) + NaBr(aq) → AgBr(s) + NaNO3(aq) c. K2S(aq) +
Write net ionic equations for the following molecular equations. HBr is a strong electrolyte. a. HBr(aq) + NH3(aq) → NH4Br(aq) b. 2HBr(aq) + Ba(OH)2(aq) → 2H2O(l) + BaBr2(aq) c. Pb(NO3)2(aq) +
Write the molecular equation and the net ionic equation for each of the following aqueous reactions. If no reaction occurs, write NR after the arrow. a. FeSO4 + NaCl → b. Na2CO3 + MgBr2 → c.
Write the molecular equation and the net ionic equation for each of the following aqueous reactions. If no reaction occurs, write NR after the arrow. a. AgNO3 + NaI → b. Ba(NO3)2 + K2SO4 → c.
For each of the following, write molecular and net ionic equations for any precipitation reaction that occurs. If no reaction occurs, indicate this.
What are the advantages and disadvantages of using a molecular equation to represent an ionic reaction?
For each of the following, write molecular and net ionic equations for any precipitation reaction that occurs. If no reaction occurs, indicate this. a. Zinc chloride and sodium sulfide are dissolved
Classify each of the following as a strong or weak acid or base.a. HFb. KOHc. HClO4d. HIO
Classify each of the following as a strong or weak acid or base. a. NH3 b. HCNO c. Sr(OH)2 d. HI
Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation. a. NaOH + HNO3 → b. HCl + Ba(OH)2 → c.
Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation. a. Al(OH)3 + HCl → b. HBr + Sr(OH)2 → c.
For each of the following, write the molecular equation, including phase labels. Then write the net ionic equation. The salts formed in these reactions are soluble.
For each of the following, write the molecular equation, including phase labels. Then write the net ionic equation. The salts formed in these reactions are soluble. Discuss.
Complete the right side of each of the following molecular equations. Then write the net ionic equations. Assume all salts formed are soluble. Acid salts are possible. a. 2KOH(aq) + H3PO4(aq) → b.
Complete the right side of each of the following molecular equations. Then write the net ionic equations. Assume all salts formed are soluble. Acid salts are possible. a. Ca(OH)2(aq) + 2H2SO4(aq)
Write molecular and net ionic equations for the successive neutralizations of each acidic hydrogen of sulfurous acid by aqueous calcium hydroxide. CaSO3 is insoluble; the acid salt is soluble.
What is a spectator ion? Illustrate with a complete ionic reaction.
Write molecular and net ionic equations for the successive neutralizations of each acidic hydrogen of phosphoric acid by calcium hydroxide solution. Ca3(PO4)2 is insoluble; assume that the acid salts
The following reactions occur in aqueous solution. Complete and balance the molecular equations using phase labels. Then write the net ionic equations. a. CaS + HBr → b. MgCO3 + HNO3 → c. K2SO3 +
The following reactions occur in aqueous solution. Complete and balance the molecular equations using phase labels. Then write the net ionic equations. a. BaCO3 + HNO3 → b. K2S + HCl → c.
Obtain the oxidation number for the element noted in each of the following. a. Ga in Ga2O3 b. Nb in NbO2 c. Br in KBrO4 d. Mn in K2MnO4
Obtain the oxidation number for the element noted in each of the following. a. Cr in CrO3 b. Hg in Hg2Cl2 c. Ga in Ga(OH)3 d. P in Na3PO4
Obtain the oxidation number for the element noted in each of the following. a. N in NH2 b. I in IO3 c. Al in Al(OH)4 d. Cl in HClO4
Obtain the oxidation number for the element noted in each of the following. a. N in NO2 b. Cr in CrO42 c. Zn in Zn(OH)42 d. As in H2AsO3
Determine the oxidation numbers of all the elements in each of the following compounds. a. Mn(ClO3)2 b. Fe2(CrO4)3 c. HgCr2O7 d. CO3(PO4)2
What is a net ionic equation? What is the value in using a net ionic equation? Give an example.
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