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chemical engineering

Fundamentals of Analytical Chemistry 9th edition Douglas A. Skoog, Donald M. West, F. James Holler, Stanley R. Crouch - Solutions

Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99 and 12.70, respectively.
Briefly describe or define and give an example of (a) An amphiprotic solute. (b) A leveling solvent.
At 25°C, what are the molar H3O+ and OH2 concentrations in? (a) 0.0300 M C6H5COOH (b) 0.100 M ethylamine (c) 0.200 M C6H5COONa (sodium benzoate) (d) 0.250 M hydroxylamine hydrochloride
At 25°C, what is the hydronium ion concentration in? (a) 0.200 M chloroacetic acid (b) 0.200 M sodium chloroacetate (c) 2.00 x 10-3 M aniline hydrochloride
Consider solutions prepared by (a) Dissolving 8.00 mmol of NaOAc in 200 mL of 0.100 M HOAc. (b) Adding 100 mL of 0.0500 M NaOH to 100 mL of 0.175 M HOAc. (c) Adding 40.0 mL of 0.1200 M HCl to 160.0 mL of 0.0420 M NaOAc. In what respects do these solutions resemble one another? How do they differ?
What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer solution that has a pH of 3.50?
What volume of 0.200 M HCl must be added to 500.0 mL of 0.300 M sodium mandelate to produce a buffer solution with a pH of 3.37?
Briefly explain why there is no term in an equilibrium constant expression for water or for a pure solid, even though one (or both) appears in the balanced net ionic equation for the equilibrium.
Identify the acid on the left and its conjugate base on the right in the following equations: (a) HOCl + H2O ⇆ H3O+ + OCl (b) NH4+ + H2O ⇆ NH3 + H3O+ (c) PO43- + H2PO4+ ⇆ 2HPO42-
Write expressions for the auto protolysis of (a) H2O. (b) CH3NH2.
Write the equilibrium-constant expressions and obtain numerical values for each constant in (a) The basic dissociation of aniline, C6H5NH2. (b) The acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. (c) The dissociation of H3AsO3 to H3O+ and AsO33-.
Generate the solubility-product expression for (a) CuBr. (b) HgClI. (c) PbCl2.
Make a distinction between (a) Activity and activity coefficient. (b) Thermodynamic and concentration equilibrium constants.
Use Equation 10-5 to calculate the activity coefficient of (a) Fe3+ at m 5 0.062. (b) Ce4+ at m 5 0.070.
For a solution in which μ = 8.0 x 10-2, calculate K'sp for(a) AgSCN.(b) La(IO3)3.
Use activities to calculate the molar solubility of Zn(OH)2 in (a) 0.0200 M KCl. (b) 0.0300 M K2SO4.
Calculate the solubilities of the following compounds in a 0.0333 M solution of Mg(ClO4)2 using (1) activities and (2) molar concentrations: (a) AgSCN. (b) PbI2. (c) BaSO4. (d) Cd2Fe(CN)6.
Calculate the solubilities of the following compounds in a 0.0167 M solution of Ba(NO3)2 using (1) activities and (2) molar concentrations: (a) AgIO3. (b) Mg(OH)2. (c) BaSO4. (d) La(IO3)3.
Calculate the % relative error in solubility by using concentrations instead of activities for the following compounds in 0.0500 M KNO3 using the thermodynamic solubility products listed in Appendix 2. (a) CuCl (aCu+ = 0.3 nm) (b) Fe (OH)3 (c) Ag3AsO4 (aAsO4 3- = 0.4 nm)
Calculate the % relative error in hydronium ion concentration by using concentrations instead of activities in calculating the pH of the following buffer solutions using the thermodynamic constants found in Appendix 3. 0.150 M HOAc and 0.250 M NaOAc
Neglecting any effects caused by volume changes, would you expect the ionic strength to (1) increase, (2) decrease, or (3) remain essentially unchanged when NaOH is added to a dilute solution of (a) Magnesium chloride [Mg(OH)2(s) forms]? (b) Hydrochloric acid? (c) Acetic acid?
Explain why the activity coefficient for dissolved ions in water is usually less than that for water itself.
Explain why the initial slope for Ca2+ in Figure 10-3 is steeper than that for K+?
Calculate the ionic strength of a solution that is (a) 0.030 M in FeSO4. (b) 0.30 M in FeCl3 and 0.20 M in FeCl2.
Calculate the molar solubility of MnS (pink) in a solution with a constant [H3O+] of 3.00 3 × 10-5
Calculate the molar solubility of ZnCO3 in a solution buffered to a pH of 7.00.
Dilute NaOH is introduced into a solution that is 0.050 M in Cu2+ and 0.040 M in Mn2+. (a) Which hydroxide precipitates first? (b) What OH- concentration is needed to initiate precipitation of the first hydroxide? (c) What is the concentration of the cation forming the less soluble hydroxide when
Silver ion is being considered for separating I- from SCN2 in a solution that is 0.040 M in KI and 0.080 M in NaSCN. (a) What Ag1 concentration is needed to lower the I2 concentration to 1.0 × 10-6 M? (b) What is the Ag+ concentration of the solution when AgSCN begins to precipitate? (c) What is
What mass of AgBr dissolves in 200 mL of 0.200 M NaCN?
Why are simplifying assumptions restricted to relationships that are sums or differences?
In contrast to many salts, calcium sulfate is only partially dissociated in aqueous solution: The solubility-product constant for CaSO4 is 2.6 × 10-5. Calculate the solubility of CaSO4 in (a) water and (b) 0.0100 M Na2SO4. In addition, calculate the percent of undissociated CaSO4 in each
Why do molar concentrations of some species appear as multiples in charge-balance equations?
Write the mass-balance expressions for a solution that is (a) 0.2 M in HF. (b) 0.10 M in H3PO4. (c) 0.0500 M in HClO2 and 0.100 M in NaClO2. (d) 0.100 M in NaOH and saturated with Zn(OH)2, which undergoes the reaction Zn(OH)2 + 2OH- ⇆ Zn(OH)42-. (e) Saturated with PbCl2.
Calculate the molar solubility of SrC2O4 in a solution that has a fixed H3O+ concentration of (a) 1.0 × 10-6 M. (b) 1.0 × 10-9 M.
Calculate the molar solubility of BaSO4 in a solution in which [H3O+] is (a) 3.5 M. (b) 0.080 M.
Calculate the molar solubility of PbS in a solution in which [H3O+] is held constant at (a) 3.0 × 10-1 M and (b) 3.0 × 10-4 M.
Explain the difference between (a) A colloidal and a crystalline precipitate. (b) Precipitation and coprecipitation. (c) Occlusion and mixed-crystal formation.
Treatment of a 0.2500-g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.2912 g of AgCl. Calculate the percentage of KCl in the sample.
What mass of Cu(IO3)2 can be formed from 0.650 g of CuSO4 ∙ 5H2O?
What mass of AgI can be produced from a 0.512-g sample that assays 20.1% AlI3?
A 0.2121-g sample of an organic compound was burned in a stream of oxygen, and the CO2 produced was collected in a solution of barium hydroxide. Calculate the percentage of carbon in the sample if 0.6006 g of BaCO3 was formed.
Define (a) Digestion. (b) Reprecipitation. (c) Counter-ion layer. (d) Supersaturation.
The mercury in a 1.0451-g sample was precipitated with an excess of paraperiodic acid, H5IO6:The precipitate was filtered, washed free of precipitating agent, dried, and weighed, and 0.5718 g was recovered. Calculate the percentage of Hg2Cl2 in the sample.
Ammoniacal nitrogen can be determined by treatment of the sample with chloroplatinic acid; the product is slightly soluble ammonium chloroplatinate:The precipitate decomposes on ignition, yielding metallic platinum and gaseous products: Calculate the percentage of ammonia in a sample if 0.2115 g
A series of sulfate samples is to be analyzed by precipitation as BaSO4. If it is known that the sulfate content in these samples ranges between 20% and 55%, what minimum sample mass should be taken to ensure that a precipitate mass no smaller than 0.200 g is produced? What is the maximum
The efficiency of a particular catalyst is highly dependent on its zirconium content. The starting material for this preparation is received in batches that assay between 68% and 84% ZrCl4. Routine analysis based on precipitation of AgCl is feasible, it having been established that there are no
A 0.6407-g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430 g. This precipitate was then strongly heated in a stream of Cl2 gas to convert the AgI to AgCl; on completion of this treatment, the precipitate weighed 0.3181 g. Calculate the percentage of
What are the structural characteristics of a chelating agent?
What mass in grams of CO2 is evolved in the complete decomposition of a 2.300-g sample that is 38.0% MgCO3 and 42.0% K2CO3 by mass?
A 50.0-mL portion of a solution containing 0.200 g of BaCl2 ∙ 2H2O is mixed with 50.0 mL of a solution containing 0.300 g of NaIO3. Assume that the solubility of Ba(IO3)2 in water is negligibly small and calculate (a) The mass of the precipitated Ba(IO3)2. (b) The mass of the unreacted compound
An aqueous solution contains NaNO3 and KBr. The bromide ion is precipitated as Ag Br by addition of AgNO3. After an excess of the precipitating reagent has been added, (a) What is the charge on the surface of the coagulated colloidal particles? (b) What is the source of the charge? (c) What ions
What is peptization and how is it avoided?
Write an equation showing how the mass of the substance sought can be converted to the mass of the weighed substance on the right.
Define (a) Millimole. (b) Stoichiometric ratio.
Calculate the molar concentration of a 20.0% solution (w/w) of KCl that has a specific gravity of 1.13
Describe the preparation of(a) 1.00 L of 0.150 M KMnO4 from the solid reagent.
A 0.4723-g sample of primary-standard-grade Na2CO3 required 34.78 mL of an H2SO4 solution to reach the end point in the reaction
A 0.4126-g sample of primary-standard Na2CO3 was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was established that 26.93 mL of the HClO4
Titration of the I2 produced from 0.1142 g of primary- standard KIO3 required 27.95 mL of sodium thiosulfate.
A 100.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00-mL of 0.002517 M K2Cr2O7 resulted in the reaction
The thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg2+ via the reaction Find the percentage of (NH2)2CS (76.12 g/mol) in the sample.
The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH: After cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate
(a) A 0.3147-g sample of primary-standard-grade Na2C2O4 was dissolved in H2SO4 and titrated with 31.67 mL of dilute KMnO4:
For each of the following acid/ base titrations, calculate the H3O+ and OH2 concentrations at equivalence and at titrant volumes corresponding to ±20.00 mL, ±10.00 mL, and 61.00 mL of equivalence. Construct a titration curve from the data, plotting the p-function versus titrant volume. (a) 25.00
Explain: The equivalence point and the end point of a titration.
Calculations of volumetric analysis ordinarily consist of transforming the quantity of titrant used (in chemical units) to a chemically equivalent quantity of analyte (also in chemical units) through use of a stoichiometric factor. Use chemical formulas (NO CALCULATIONSREQUIRED) to express this
How many millimoles of solute are contained in (a) 2.95 mL of 0.0789 M KH2PO4? (b) 0.2011 L of 0.0564 M HgCl2?
What mass of solute in grams is contained in (a) 450.0 mL of 0.0986 M H2O2? (b) 26.4 mL of 9.36 × 10-4 M benzoic acid (122.1 g/ mol)?
Why does the typical acid/base indicator exhibit its color change over a range of about 2 pH units?
Using the data in Problem 14-10, calculate the pH of a 1.00 × 10-2 M NaOH solution at 508C.
What is the pH of an aqueous solution that is 3.00% HCl by mass and has a density of 1.015 g/mL?
What is the pH of a solution that is 2.00 × 10-8 M in NaOH?
What is the pH of the solution that results when 0.093 g of Mg(OH)2 is mixed with (a) 75.0 mL of 0.0500 M HCl? (b) 100.0 mL of 0.0500 M HCl? (c) 15.0 mL of 0.0500 M HCl? (d) 30.0 mL of 0.0500 M MgCl2?
Calculate the hydronium ion concentration and pH of a solution that is 0.0500 M in HCl (a) Neglecting activities. (b) Using activities.
Calculate the pH of an aqueous solution that is(a) 1.00 × 10-1 M in HOCl.(b) 1.00 × 10-2 M in HOCl.(c) 1.00 × 10-4 M HOCl.
Calculate the pH of an ammonia solution that is (a) 1.00 × 10-1 M NH3. (b) 1.00 × 10-2 M NH3. (c) 1.00 × 10-4 M NH3.
Calculate the pH of a solution in which the concentration of piperdine is (a) 1.00 × 10-1 M. (b) 1.00 × 10-2 M. (c) 1.00 × 10-4 M.
Calculate the pH of a solution prepared by (a) Dissolving 36.5 g of lactic acid in water and diluting to 500 mL. (b) Diluting 25.0 mL of the solution in (a) to 250 mL. (c) Diluting 10.0 mL of the solution in (b) to 1.00 L.
Calculate the pH of the solution that results when 20.0 mL of 0.1750 M formic acid is (a) Diluted to 45.0 mL with distilled water. (b) Mixed with 25.0 mL of 0.140 M NaOH solution. (c) Mixed with 25.0 mL of 0.200 M NaOH solution. (d) Mixed with 25.0 mL of 0.200 sodium formate
Consider curves for the titration of 0.10 M NaOH and 0.010 M NH3 with 0.10 M HCl. (a) Briefly account for the differences between curves for the two titrations. (b) In what respect will the two curves be indistinguishable?
A solution is 0.0500 M in NH4Cl and 0.0300 M in NH3. Calculate its OH2 concentration and its pH (a) Neglecting activities. (b) Taking activities into account.
What is the pH of a solution that is(a) Prepared by dissolving 3.30 g of (NH4)2SO4 in water, adding 125.0 mL of 0.1011 M NaOH, and diluting to 500.0 mL?(b) 0.120 M in piperidine and 0.010 M in its chloride salt?(c) 0.050 M in ethylamine and 0.167 M in its chloride salt?(d) Prepared by dissolving
Calculate the change in pH that occurs in each of the solutions listed below as a result of a tenfold dilution with water. Round calculated values for pH to three figures to the right of the decimal point. (a) H2O. (b) 0.0500 M NaOH. (c) 0.0500 M CH3COONa. (d) 0.500 M CH3COOH + 0.500 M CH3COONa.
Calculate the change in pH that occurs when 1.00 mmol of a strong acid is added to 100 mL of the solutions listed in Problem 14-34. In Problem 14.34 (a) H2O. (b) 0.0500 M HCl. (c) 0.0500 M NaOH. (d) 0.0500 M CH3COOH. (e) 0.0500 M CH3COONa. (f) 0.0500 M CH3COOH + 0.0500 M CH3COONa. (g) 0.500 M
Calculate the change in pH to three decimal places that occurs when 0.50 mmol of a strong acid is added to 100 mL of (a) 0.0200 M lactic acid + 0.0800 M sodium lactate. (b) 0.0800 M lactic acid + 0.0200 M sodium lactate. (c) 0.0500 M lactic acid + 0.0500 M sodium lactate.
Calculate α0 and α1 for
Calculate the equilibrium concentration of methyl ammonia in a solution that has a molar analytical CH3NH2 concentration of 0.120 and a pH of 11.471.
Supply the missing data in the table below.
Which solute would provide the sharper end point in a titration with 0.10 M HCl:(a) 0.10 M NaOCl or 0.10 M hydroxylamine?(b) 0.10 M methylamine or 0.10 M hydroxylamine?
Which solute would provide the sharper end point in a titration with 0.10 M NaOH: (a) 0.10 M nitrous acid or 0.10 M iodic acid? (b) 0.10 M hypochlorous acid or 0.10 M pyruvic acid?
The procedure described in Problem 14-8 was used to determine pH with methyl orange as the indicator. The concentration ratio of the acid to base form of the indicator was 1.84. Calculate the pH of the solution.
As its name implies, NaHA is an "acid salt" because it has a proton available to donate to a base. Briefly explain why a pH calculation for a solution of NaHA differs from that for a weak acid of the type HA.
Calculate the pH of a solution that is 0.0400 M in *(a) NaH2PO4. (b) NaHC2O4. *(c) NaH2PO3. (d) NaHSO3. *(e) NaHS. (f) H2NC2H4NH3 +CI-
Calculate the pH of a solution that is 0.0400 M in *(a) Na3PO4. (b) Na2C2O4. *(c) Na2HPO3. (d) Na2SO3. *(e) Na2S. (f) C2H4(NH3+CI-)2.
Calculate the pH of a solution that contains the following analytical concentrations: (a) 0.225 M in H3PO4 and 0.414 M in NaH2PO4. (b) 0.0670 M in Na2SO3 and 0.0315 M in NaHSO3. (c) 0.640 M in HOC2H4NH2 and 0.750 M in HOC2H4NH3Cl. (d) 0.0240 in H2C2O4 (oxalic acid) and 0.0360 M in Na2C2O4. (e)
Calculate the pH of a solution that is (a) 0.0100 M in HClO4 and 0.0300 M in monochloroacetic acid. (b) 0.0100 M in HCl and 0.0150 M in H2SO4. (c) 0.0100 M in NaOH and 0.0300 M in Na2S. (d) 0.0100 M in NaOH and 0.0300 M in sodium
Identify the principal conjugate acid/base pair and calculate the ratio between them in a solution that is buffered to pH 9.00 and contains (a) H2S. (b) Ethylenediamine dihydrochloride. (c) H3AsO4. (d) H2CO3.
What mass (g) of dipotassium phthalate must be added to 750 mL of 0.0500 M phthalic acid to give a buffer of pH 5.75?
What is the pH of the buffer formed by adding 100 mL of 0.150 M potassium hydrogen phthalate to (a) 100.0 mL of 0.0800 M NaOH? (b) 100.0 mL of 0.0800 M HCl?

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