Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Chapter 15, Problem 86QRT
Interpretation Introduction
Interpretation:
The mass of ammonium chloride required to prepare a buffer of
Concept Introduction:
The buffer is a solution that resists any change in pH on addition of
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Chemistry: The Molecular Science
Ch. 15.1 - Predict whether 1.0 L of each solution is a...Ch. 15.1 - Calculate the pH of blood containing 0.0020-M...Ch. 15.1 - Prob. 15.2ECh. 15.1 -
Calculate the ratio of [] to [] in blood at a...Ch. 15.1 - Use the data in Table 15.1 to select a conjugate...Ch. 15.1 -
Calculate the mole ratio of sodium acetate and...Ch. 15.1 - Calculate the pH of these buffers.
Ch. 15.1 - If an abnormally high CO2 concentration is present...Ch. 15.1 - Calculate the minimum mass (g) of KOH that would...Ch. 15.2 - For the titration of 50.0 mL of 0.100-M HCl with...
Ch. 15.2 - Draw the titration curve for the titration of 50.0...Ch. 15.2 - Use the Ka expression and value for acetic acid to...Ch. 15.2 - Explain why the curve for the titration of acetic...Ch. 15.4 - Write the Ksp expression for each of these...Ch. 15.4 - The Ksp of AgBr at 100 C is 5 1010. Calculate the...Ch. 15.4 - A saturated solution of silver oxalate. Ag2C2O4....Ch. 15.4 - Prob. 15.9CECh. 15.5 - Consider 0.0010-M solutions of these sparingly...Ch. 15.5 - Prob. 15.11PSPCh. 15.5 - Calculate the solubility of PbCl2 in (a) pure...Ch. 15.5 - Prob. 15.13PSPCh. 15.6 - (a) Determine whether AgCl precipitates from a...Ch. 15.6 - Prob. 15.15PSPCh. 15 - Prob. 1SPCh. 15 - Choose a weak-acid/weak-base conjugate pair from...Ch. 15 - Prob. 4SPCh. 15 - Define the term buffer capacity.Ch. 15 - What is the difference between the end point and...Ch. 15 - What are the characteristics of a good acid-base...Ch. 15 - A strong acid is titrated with a strong base, such...Ch. 15 - Repeat the description for Question 4, but use a...Ch. 15 - Use Le Chatelier’s principle to explain why PbCl2...Ch. 15 - Describe what a complex ion is and give an...Ch. 15 - Define the term “amphoteric”.
Ch. 15 - Distinguish between the ion product (Q) expression...Ch. 15 - Describe at least two ways that the solubility of...Ch. 15 - Briefly describe how a buffer solution can control...Ch. 15 - Identify each pair that could form a buffer. (a)...Ch. 15 - Identify each pair that could form a buffer. (a)...Ch. 15 - Many natural processes can be studied in the...Ch. 15 - Which of these combinations is the best to buffer...Ch. 15 - Without doing calculations, determine the pH of a...Ch. 15 - Without doing calculations, determine the pH of a...Ch. 15 - Select from Table 15.1 a conjugate acid-base pair...Ch. 15 - Select from Table 15.1 a conjugate acid-base pair...Ch. 15 - Calculate the mass of sodium acetate, NaCH3COO,...Ch. 15 - Calculate the mass in grams of ammonium chloride,...Ch. 15 - A buffer solution can be made from benzoic acid,...Ch. 15 - A buffer solution is prepared from 5.15 g NH4NO3...Ch. 15 - You dissolve 0.425 g NaOH in 2.00 L of a solution...Ch. 15 - A buffer solution is prepared by adding 0.125 mol...Ch. 15 - If added to 1 L of 0.20-M acetic acid, CH3COOH,...Ch. 15 - If added to 1 L of 0.20-M NaOH, which of these...Ch. 15 - Calculate the pH change when 10.0 mL of 0.100-M...Ch. 15 - Prob. 29QRTCh. 15 - Prob. 30QRTCh. 15 - Prob. 31QRTCh. 15 - The titration curves for two acids with the same...Ch. 15 - Explain why it is that the weaker the acid being...Ch. 15 - Prob. 34QRTCh. 15 - Consider all acid-base indicators discussed in...Ch. 15 - Which of the acid-base indicators discussed in...Ch. 15 - It required 22.6 mL of 0.0140-M Ba(OH)2 solution...Ch. 15 - It took 12.4 mL of 0.205-M H2SO4 solution to...Ch. 15 - Vitamin C is a monoprotic acid. To analyze a...Ch. 15 - An acid-base titration was used to find the...Ch. 15 - Calculate the volume of 0.150-M HCl required to...Ch. 15 - Calculate the volume of 0.225-M NaOH required to...Ch. 15 - Prob. 43QRTCh. 15 - Prob. 44QRTCh. 15 - Prob. 45QRTCh. 15 - Explain why rain with a pH of 6.7 is not...Ch. 15 - Identify two oxides that are key producers of acid...Ch. 15 - Prob. 48QRTCh. 15 - Prob. 49QRTCh. 15 - Prob. 50QRTCh. 15 - Prob. 51QRTCh. 15 - A saturated solution of silver arsenate, Ag3AsO4,...Ch. 15 - Prob. 53QRTCh. 15 - Prob. 54QRTCh. 15 - Prob. 55QRTCh. 15 - Prob. 56QRTCh. 15 - Prob. 57QRTCh. 15 - Prob. 58QRTCh. 15 - Prob. 59QRTCh. 15 - Prob. 60QRTCh. 15 - Prob. 61QRTCh. 15 - Prob. 62QRTCh. 15 - Prob. 63QRTCh. 15 - Prob. 64QRTCh. 15 - Predict what effect each would have on this...Ch. 15 - Prob. 66QRTCh. 15 - Prob. 67QRTCh. 15 - The solubility of Mg(OH)2 in water is...Ch. 15 - Prob. 69QRTCh. 15 - Prob. 70QRTCh. 15 - Prob. 71QRTCh. 15 - Prob. 72QRTCh. 15 - Write the chemical equation for the formation of...Ch. 15 - Prob. 74QRTCh. 15 - Prob. 75QRTCh. 15 - Prob. 76QRTCh. 15 - Prob. 77QRTCh. 15 - Prob. 78QRTCh. 15 - Prob. 79QRTCh. 15 - Prob. 80QRTCh. 15 - Prob. 81QRTCh. 15 - Solid sodium fluoride is slowly added to an...Ch. 15 - Prob. 83QRTCh. 15 - Prob. 84QRTCh. 15 - A buffer solution was prepared by adding 4.95 g...Ch. 15 - Prob. 86QRTCh. 15 - Prob. 87QRTCh. 15 - Prob. 88QRTCh. 15 - Prob. 89QRTCh. 15 - Which of these buffers involving a weak acid HA...Ch. 15 - Prob. 91QRTCh. 15 - Prob. 92QRTCh. 15 - When 40.00 mL of a weak monoprotic acid solution...Ch. 15 - Each of the solutions in the table has the same...Ch. 15 - Prob. 95QRTCh. 15 - Prob. 97QRTCh. 15 - The average normal concentration of Ca2+ in urine...Ch. 15 - Explain why even though an aqueous acetic acid...Ch. 15 - Prob. 100QRTCh. 15 - Prob. 101QRTCh. 15 - Prob. 102QRTCh. 15 - Prob. 103QRTCh. 15 - Prob. 104QRTCh. 15 - Apatite, Ca5(PO4)3OH, is the mineral in teeth.
On...Ch. 15 - Calculate the maximum concentration of Mg2+...Ch. 15 - Prob. 107QRTCh. 15 - Prob. 108QRTCh. 15 - The grid has six lettered boxes, each of which...Ch. 15 - Consider the nanoscale-level representations for...Ch. 15 - Consider the nanoscale-level representations for...Ch. 15 - Prob. 112QRTCh. 15 - Prob. 113QRTCh. 15 - Prob. 114QRTCh. 15 - Prob. 115QRTCh. 15 - You want to prepare a pH 4.50 buffer using sodium...Ch. 15 - Prob. 117QRTCh. 15 - Prob. 118QRTCh. 15 - Prob. 119QRTCh. 15 - Prob. 120QRTCh. 15 - Prob. 121QRTCh. 15 - Prob. 122QRTCh. 15 - You are given four different aqueous solutions and...Ch. 15 - Prob. 124QRTCh. 15 - Prob. 126QRTCh. 15 - Prob. 15.ACPCh. 15 - Prob. 15.BCP
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- Calculate the mass of sodium acetate, NaCH3COO, you should add to 500. mL of a 0.150-M solution of acetic acid, CH3COOH, to buffer a solution at a pH of 4.57.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_forwardHow many grams of NaF must be added to 70.00 mL of 0.150 M HNO3 to obtain a buffer with a pH of 4.68?arrow_forward
- Ka 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 buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardThe species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?arrow_forward
- Ammonia 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_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_forwardA 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?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_forwardYou want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?arrow_forwardA 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_forward
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