Chemistry: Atoms First V1
1st Edition
ISBN: 9781259383120
Author: Burdge
Publisher: McGraw Hill Custom
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Chapter 17, Problem 17.2QP
Describe the effect on pH (increase, decrease, or no change) that results from each of the following additions: (a) potassium acetate to an acetic acid solution, (b) ammonium nitrate to an ammonia solution, (c) sodium formate (HCOONa) to a formic acid (HCOOH) solution, (d) potassium chloride to a hydrochloric acid solution, (e) barium iodide to a hydroiodic acid solution.
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The acidity of a solution is measured by its pH.
If HT| represents the concentration of hydrogen ions (in moles/liter) in the solution,
the pH is defined by pH = – log H+
Based on careful measurements and calculations, a chemist examines two solutions and asserts:
"The hydrogen ion concentration of Solution A
is 37.93% greater than the hydrogen ion concentration of Solution B."
If the pH of solution B is 4.36, determine the pH of Solution A.
Report your answer to two decimal places.
Solution A has pH equal to
Number
- (Report to the nearest 0.01)
A buffer solution was made by mixing 2.00 L of 1.500 M potassium nitrite with 1.00 L of 1.476 M nitrous acid.
Ka (nitrous acid) = 4.5 x 10-4
For all to the following questions, write your answer as a normal number to three significant figures.
(a) The molarity of the conjugate base in the solution at the instant of mixing is
(b) The molarity of the weak acid in the solution at the instant of mixing is
(c) The pH of the buffer after the mixing of the two solutions is
Use the rules applicable to significant figures.
(d) 19.04 g NaOH (39.9971 g/mol) is dissolved in this buffer solution (assume this causes no change in the volume of the solution) and reacts. The mole of
added base remaining after the reaction is
(e) At the same time, the moles of weak acid remaining is
(f) At the same time, the moles of the conjugate base remaining is
(9) THe pH of the buffer solution after the added base has reacted, is
Use the rules applicable to significant figures.
Red cabbage juice is a sensitive acid-base indicator; its colors range from red at acidic pH to yellow in alkaline solutions. If red cabbage is used for the following titration, calculate the pH of the solution described and indicate whether the solution will be red or yellow.
If 67.00 mL of a 1.980 M HNO2 solution is reacted with 2.350 g NaOH, calculate the resulting pH.
Resulting pH =
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Chapter 17 Solutions
Chemistry: Atoms First V1
Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Prob. 1PPCCh. 17.1 - Prob. 17.1.1SRCh. 17.1 - Prob. 17.1.2SRCh. 17.2 - Starting with 1.00 L of a buffer that is 1.00 M in...Ch. 17.2 - Prob. 2PPACh. 17.2 - Prob. 2PPBCh. 17.2 - Prob. 2PPC
Ch. 17.2 - Prob. 17.3WECh. 17.2 - Prob. 3PPACh. 17.2 - Prob. 3PPBCh. 17.2 - Prob. 3PPCCh. 17.2 - Prob. 17.2.1SRCh. 17.2 - Prob. 17.2.2SRCh. 17.2 - Prob. 17.2.3SRCh. 17.2 - Prob. 17.2.4SRCh. 17.3 - Calculate the pH in the titration of 50.0 mL of...Ch. 17.3 - For the titration of 10.0 mL of 0.15 M acetic acid...Ch. 17.3 - Prob. 4PPBCh. 17.3 - Prob. 4PPCCh. 17.3 - Prob. 17.5WECh. 17.3 - Prob. 5PPACh. 17.3 - Prob. 5PPBCh. 17.3 - Which of the graphs [(i)(iv)] best represents the...Ch. 17.3 - Prob. 17.6WECh. 17.3 - Prob. 6PPACh. 17.3 - Prob. 6PPBCh. 17.3 - Prob. 6PPCCh. 17.3 - Prob. 17.3.1SRCh. 17.3 - Prob. 17.3.2SRCh. 17.3 - Prob. 17.3.3SRCh. 17.4 - Calculate the solubility of copper(II) hydroxide...Ch. 17.4 - Calculate the molar solubility and the solubility...Ch. 17.4 - Calculate the molar solubility and the solubility...Ch. 17.4 - Prob. 7PPCCh. 17.4 - Prob. 17.8WECh. 17.4 - Prob. 8PPACh. 17.4 - Prob. 8PPBCh. 17.4 - Prob. 8PPCCh. 17.4 - Prob. 17.9WECh. 17.4 - Predict whether a precipitate will form from each...Ch. 17.4 - Prob. 9PPBCh. 17.4 - Prob. 9PPCCh. 17.4 - Prob. 17.4.1SRCh. 17.4 - Prob. 17.4.2SRCh. 17.4 - Prob. 17.4.3SRCh. 17.5 - Prob. 17.10WECh. 17.5 - Calculate the molar solubility of AgI in (a) pure...Ch. 17.5 - Arrange the following salts in order of increasing...Ch. 17.5 - Prob. 17.11WECh. 17.5 - Determine if the following compounds are more...Ch. 17.5 - Prob. 11PPBCh. 17.5 - Prob. 11PPCCh. 17.5 - Prob. 17.12WECh. 17.5 - Prob. 12PPACh. 17.5 - Prob. 12PPBCh. 17.5 - Beginning with a saturated solution of AgCl, which...Ch. 17.5 - Prob. 17.5.1SRCh. 17.5 - Prob. 17.5.2SRCh. 17.6 - Prob. 17.13WECh. 17.6 - Prob. 13PPACh. 17.6 - Prob. 13PPBCh. 17.6 - Prob. 13PPCCh. 17.6 - Prob. 17.6.1SRCh. 17.6 - Prob. 17.6.2SRCh. 17 - Use Le Chteliers principle to explain how the...Ch. 17 - Describe the effect on pH (increase, decrease, or...Ch. 17 - Prob. 17.3QPCh. 17 - Prob. 17.4QPCh. 17 - Determine the pH of (a) a 0.40 M CH3COOH solution,...Ch. 17 - Determine the pH of (a) a 0.20 M NH3 solution, and...Ch. 17 - Which pair of substances can be dissolved together...Ch. 17 - Prob. 17.2VCCh. 17 - Prob. 17.3VCCh. 17 - Prob. 17.4VCCh. 17 - Prob. 17.7QPCh. 17 - Prob. 17.8QPCh. 17 - Calculate the pH of the buffer system made up of...Ch. 17 - Calculate the pH of the following two buffer...Ch. 17 - Prob. 17.11QPCh. 17 - Prob. 17.12QPCh. 17 - Prob. 17.13QPCh. 17 - The pH of blood plasma is 7.40. Assuming the...Ch. 17 - Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl...Ch. 17 - Calculate the pH of 1.00 L of the buffer 1.00 M...Ch. 17 - Prob. 17.17QPCh. 17 - Prob. 17.18QPCh. 17 - Prob. 17.19QPCh. 17 - Prob. 17.20QPCh. 17 - The diagrams [(a)(d)] contain one or more of the...Ch. 17 - Prob. 17.22QPCh. 17 - Prob. 17.23QPCh. 17 - Prob. 17.24QPCh. 17 - Prob. 17.25QPCh. 17 - The amount of indicator used in an acid-base...Ch. 17 - Prob. 17.27QPCh. 17 - Prob. 17.28QPCh. 17 - Prob. 17.29QPCh. 17 - Prob. 17.30QPCh. 17 - Prob. 17.31QPCh. 17 - Prob. 17.32QPCh. 17 - Prob. 17.33QPCh. 17 - Prob. 17.34QPCh. 17 - A 25.0-,L solution of 0n100 M CH3COOH is titrated...Ch. 17 - A 10.0-mL solution of 0.300 M NH3 is titratee with...Ch. 17 - Prob. 17.37QPCh. 17 - Prob. 17.38QPCh. 17 - Prob. 17.39QPCh. 17 - Prob. 17.40QPCh. 17 - Diagrams (a) through (d) represent solutions at...Ch. 17 - Prob. 17.42QPCh. 17 - Prob. 17.43QPCh. 17 - Prob. 17.44QPCh. 17 - Write balanced equations and solubility product...Ch. 17 - Prob. 17.46QPCh. 17 - Prob. 17.47QPCh. 17 - Prob. 17.48QPCh. 17 - Prob. 17.49QPCh. 17 - Prob. 17.50QPCh. 17 - Prob. 17.51QPCh. 17 - The solubility of an ionic compound MX (molar mass...Ch. 17 - Prob. 17.53QPCh. 17 - Prob. 17.54QPCh. 17 - Prob. 17.55QPCh. 17 - Prob. 17.56QPCh. 17 - Prob. 17.57QPCh. 17 - A volume of 75 mL of 0.060 M NaF is mixed with 25...Ch. 17 - Prob. 17.59QPCh. 17 - Prob. 17.60QPCh. 17 - Prob. 17.5VCCh. 17 - Prob. 17.6VCCh. 17 - Prob. 17.7VCCh. 17 - How would the concentration of silver ion in the...Ch. 17 - Prob. 17.61QPCh. 17 - Prob. 17.62QPCh. 17 - Prob. 17.63QPCh. 17 - Prob. 17.64QPCh. 17 - The solubility product of PbBr2 is 8.9 106....Ch. 17 - Prob. 17.66QPCh. 17 - Calculate the molar solubility of BaSO4 in (a)...Ch. 17 - Prob. 17.68QPCh. 17 - Prob. 17.69QPCh. 17 - Prob. 17.70QPCh. 17 - Prob. 17.71QPCh. 17 - Prob. 17.72QPCh. 17 - Calculate the concentrations of Cd2+, Cd(CN)42 ,...Ch. 17 - Prob. 17.74QPCh. 17 - Prob. 17.75QPCh. 17 - (a) Calculate the molar solubility of...Ch. 17 - Prob. 17.77QPCh. 17 - Prob. 17.78QPCh. 17 - Prob. 17.79QPCh. 17 - Prob. 17.80QPCh. 17 - Prob. 17.81QPCh. 17 - Prob. 17.82QPCh. 17 - Prob. 17.83QPCh. 17 - Prob. 17.84QPCh. 17 - In a group 1 analysis, a student adds HCl acid to...Ch. 17 - Prob. 17.86QPCh. 17 - Prob. 17.87QPCh. 17 - Sketch the titration curve of a weak acid with a...Ch. 17 - Prob. 17.89QPCh. 17 - Prob. 17.90QPCh. 17 - Prob. 17.91QPCh. 17 - Tris [tris(hydroxymethyl)aminomethane] is a common...Ch. 17 - Prob. 17.93QPCh. 17 - Prob. 17.94QPCh. 17 - Prob. 17.95QPCh. 17 - Prob. 17.96QPCh. 17 - Prob. 17.97QPCh. 17 - Find the approximate pH range suitable for...Ch. 17 - Prob. 17.99QPCh. 17 - Prob. 17.100QPCh. 17 - Prob. 17.101QPCh. 17 - Prob. 17.102QPCh. 17 - Barium is a toxic substance that can seriously...Ch. 17 - The pKa of phenolphthalein is 9.10. Over what pH...Ch. 17 - Prob. 17.105QPCh. 17 - Prob. 17.106QPCh. 17 - Prob. 17.107QPCh. 17 - The molar mass of a certain metal carbonate, MCO3,...Ch. 17 - Prob. 17.109QPCh. 17 - Prob. 17.110QPCh. 17 - Describe how you would prepare a 1 -L 0.20 M...Ch. 17 - Phenolphthalein is the common indicator for the...Ch. 17 - Prob. 17.113QPCh. 17 - Prob. 17.114QPCh. 17 - Prob. 17.115QPCh. 17 - Prob. 17.116QPCh. 17 - Prob. 17.117QPCh. 17 - Prob. 17.118QPCh. 17 - When lemon juice is added to tea, the color...Ch. 17 - How many milliliters of 1.0 M NaOH must be added...Ch. 17 - Prob. 17.121QPCh. 17 - Prob. 17.122QPCh. 17 - Prob. 17.123QPCh. 17 - Prob. 17.124QPCh. 17 - Calcium oxalate is a major component of kidney...Ch. 17 - Water containing Ca2+ and Mg2+ ions is called hard...Ch. 17 - Prob. 17.127QPCh. 17 - Prob. 17.128QPCh. 17 - Prob. 17.129QPCh. 17 - (a) Referring to Figure 17.4, describe how you...Ch. 17 - Prob. 17.131QPCh. 17 - Prob. 17.132QPCh. 17 - Prob. 17.133QPCh. 17 - Prob. 17.134QPCh. 17 - Prob. 17.135QPCh. 17 - Prob. 17.136QPCh. 17 - A sample of 0.96 L of HCl gas at 372 mmHg and 22C...Ch. 17 - Prob. 17.138QPCh. 17 - The solutions (a) through (f) represent various...Ch. 17 - Prob. 17.140QPCh. 17 - Prob. 17.141QPCh. 17 - Which of the acids in Table 16.5 (page 732) can be...Ch. 17 - Prob. 17.2KSPCh. 17 - Prob. 17.3KSPCh. 17 - How much sodium fluoride must be dissolved in 250...
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