Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 15, Problem 11QAP
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
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Chapter 15 Solutions
Chemistry: Principles and Reactions
Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Calculate K for the reactions in Question 1.Ch. 15 - Calculate K for the reactions in Question 2.Ch. 15 - Calculate K for the reactions in Question 3.Ch. 15 - Calculate K for the reactions in Question 4.Ch. 15 - Calculate [H+] and pH in a solution in which...Ch. 15 - Calculate [OH-] and pH in a solution in which the...
Ch. 15 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 15 - Prob. 12QAPCh. 15 - A buffer solution is prepared by adding 15.00 g of...Ch. 15 - A buffer solution is prepared by adding 5.50 g of...Ch. 15 - A solution with a pH of 9.22 is prepared by adding...Ch. 15 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Copper(l) chloride, CuCl, is the starting material...Ch. 15 - Prob. 22QAPCh. 15 - Prob. 23QAPCh. 15 - Ksp for CaSO4 at 100C is estimated to be1.6105. At...Ch. 15 - Prob. 25QAPCh. 15 - At 25C, 10.24 mg of Cr(OH)2 are dissolved in...Ch. 15 - Calcium nitrate is added to a sodium sulfate...Ch. 15 - Cadmium(ll) chloride is added to a solution of...Ch. 15 - Water from a well is found to contain 3.0 mg of...Ch. 15 - Silver(I) sulfate (Ksp=1.2105) is used in the...Ch. 15 - A solution is prepared by mixing 13.00 mL of...Ch. 15 - A solution is prepared by mixing 45.00 mL of 0.022...Ch. 15 - A solution is 0.047 M in both NaF and Na2CO3....Ch. 15 - Solid lead nitrate is added to a solution that is...Ch. 15 - A solution is made up by adding 0.632 g of barium...Ch. 15 - A solution is made up by adding 0.839 g of...Ch. 15 - Prob. 37QAPCh. 15 - To a beaker with 500 mL of water are added 95 mg...Ch. 15 - Write net ionic equations for the reaction of H+...Ch. 15 - Prob. 40QAPCh. 15 - Prob. 41QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 43QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 45QAPCh. 15 - Write an overall net ionic equation and calculate...Ch. 15 - Consider the reaction...Ch. 15 - Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2...Ch. 15 - Aluminum hydroxide reacts with an excess of...Ch. 15 - Prob. 50QAPCh. 15 - Calculate the molar solubility of gold(I) chloride...Ch. 15 - Calculate the molar solubility of PbCl2 in 0.2 M...Ch. 15 - For the reaction...Ch. 15 - For the reaction Zn(OH)2(s)+2OH(aq)Zn(OH)42(aq)...Ch. 15 - What are the concentrations of Cu2+, NH3, and...Ch. 15 - Prob. 56QAPCh. 15 - Calcium ions in blood trigger clotting. To prevent...Ch. 15 - Prob. 58QAPCh. 15 - A town adds 2.0 ppm of F- ion to fluoridate its...Ch. 15 - Consider the following hypothetical dissociation:...Ch. 15 - Prob. 61QAPCh. 15 - Consider a 2.0-L aqueous solution of 4.17 M NH3,...Ch. 15 - Marble is almost pure CaCO3. Acid rain has a...Ch. 15 - Prob. 64QAPCh. 15 - Prob. 65QAPCh. 15 - The box below represents one liter of a saturated...Ch. 15 - Consider a saturated solution of BaCO3 at 7.5C....Ch. 15 - Prob. 68QAPCh. 15 - Consider the insoluble salts JQ, K2R, L2S3, MT2,...Ch. 15 - Prob. 70QAPCh. 15 - Consider the equilibrium curve for AgCl shown...Ch. 15 - Dissolving CaCO3 is an endothermic reaction. The...Ch. 15 - Challenge Problems Insoluble hydroxides such as...Ch. 15 - What is the solubility of CaF2 in a buffer...Ch. 15 - What is [Br-] just as AgCl begins to precipitate...Ch. 15 - Prob. 76QAPCh. 15 - Prob. 77QAPCh. 15 - Prob. 78QAP
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- A buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.arrow_forwardKa for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.arrow_forwardA solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.arrow_forward
- A buffer solution is prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.arrow_forwardAmmonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.arrow_forwardA buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.arrow_forward
- A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)arrow_forwardA buffer is prepared by mixing 525 mL of 0.50 M formic acid, HCHO2, and 475 mL of 0.50 M sodium formate, NaCHO2. Calculate the pH. What would be the pH of 85 mL of the buffer to which 8.6 mL of 0.15 M hydrochloric acid had been added?arrow_forwardThe pH of 0.10 M CH3NH2 (methylamine) is 11.8. When the chloride salt of methylamine, CH3NH3Cl, is added to this solution, does the pH increase or decrease? Explain, using Le Chteliers principle and the common-ion effect.arrow_forward
- Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.arrow_forwardWhen 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.arrow_forwardWithout doing calculations, determine the pH of a buffer made front equimolar amounts of these acid-base pairs. (a) Nitrous acid and sodium nitrite (b) Ammonia and ammonium chloride (c) Formic acid and potassium formatearrow_forward
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