Chemistry: Central Science - Package (Custom)
13th Edition
ISBN: 9781269703741
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 3.4, Problem 3.11.2PE
Practice Exercise 2
Calculate the format ion concentration and pH of a solution that is 0.050 M in formic acid (HCOOH, Ka= 1.8 X 10-4 ) and 0.10 M in HNO3.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
pH practice
a.) determine the pH of a nitric acid solution (HNO3) that has been prepared by mixing 2.0 mL of 1.0 M HNO3 with 98.0 mL of water
b.) determine the pH of a 25 mL carbonic acid solution (H2CO3) with a concentration of 5.7 x 10-5 M. assume all the protons will dissociate from the acid and react with water to form hydronium ions.
c.) determine the pH and pOH of a NaOH solution that has been prepared by diluting 20.0 mL of 6.0 M NaOH with 80.0 mL of water.
d.) determine the pH and pOH of a Ca(OH)2 solution that has been prepared by mixing 0.26 g of Ca(OH)2 pellets in 750 mL of water.
Learning Check Determine the pH of a 0.1M solution of the salt NaF basic due to F- Kb=Kw/Ka UNIVERSITY x² / 0.1 = 2.87e-11 I C F- 0.1M -X + H₂O → OH- + HF (aq) aq. E (0.1-x)≈ 0.1 N/A -X • N/A pOH=? 0 +x X 16.3. Salt solutions are not neutral if the ions are weak acids or bases pH=? 0 +x
Homework:
Answer the following:
Determine the pH level of a solution that has 0.02372 M of Formic acid, given that the Ka of formic acid is equal to 1.400 x 10-4
Chapter 3 Solutions
Chemistry: Central Science - Package (Custom)
Ch. 3.1 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 3.1 - Prob. 3.1.2PECh. 3.1 - Consider a saturated solution of the salt MA3, in...Ch. 3.1 - Prob. 3.2.2PECh. 3.2 - Prob. 3.3.1PECh. 3.2 - Prob. 3.3.2PECh. 3.2 - Prob. 3.4.1PECh. 3.2 - Prob. 3.4.2PECh. 3.3 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 3.3 - Does a precipitate form when 0.050 L of 2.0 × 10-2...
Ch. 3.3 - Under what conditions does an ionic compound...Ch. 3.3 - Prob. 3.6.2PECh. 3.4 - Prob. 3.7.1PECh. 3.4 - The following boxes represent aqueos solutions...Ch. 3.4 - Prob. 3.8.1PECh. 3.4 - Prob. 3.8.2PECh. 3.4 - Prob. 3.9.1PECh. 3.4 - Prob. 3.9.2PECh. 3.4 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 3.4 - Practice Exercise 2 Calculate the pH of a solution...Ch. 3.4 - Calculate the concentration of the lactate ion in...Ch. 3.4 - Practice Exercise 2 Calculate the format ion...Ch. 3.4 - Practice Exercise 1 If the pH of a buffer solution...Ch. 3.4 - Prob. 3.12.2PECh. 3.5 - Prob. 3.13.1PECh. 3.5 - Prob. 3.13.2PECh. 3.5 - Calculate the number of grams of ammonium chloride...Ch. 3.5 - Prob. 3.14.2PECh. 3.5 - Prob. 3.15.1PECh. 3.5 - Determine The pH of the original buffer described...Ch. 3.6 - An acid-base titration is performed: 250.0 mL of...Ch. 3.6 - Prob. 3.16.2PECh. 3.6 - Prob. 3.17.1PECh. 3.6 - Calculate the pH in the solution formed by adding...Ch. 3.7 - Prob. 3.18.1PECh. 3.7 - Prob. 3.18.2PECh. 3.7 - Prob. 3.19.1PECh. 3.7 - Prob. 3.19.2PECh. 3.7 - Prob. 3.20.1PECh. 3.7 - Prob. 3.20.2PECh. 3 - The accompanying graph shows the titration curves...Ch. 3 - Prob. 2ECh. 3 - Prob. 3ECh. 3 - Prob. 4ECh. 3 - Prob. 5ECh. 3 - Prob. 6ECh. 3 - Prob. 7ECh. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Use information from Appendix D to calculate the...Ch. 3 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 3 - You are asked to prepare a pH = 3.00 buffer...Ch. 3 - You are asked to prepare an pH = 4.00 buffer...Ch. 3 - Prob. 14ECh. 3 - Prob. 15ECh. 3 - Prob. 16ECh. 3 - Prob. 17ECh. 3 - Prob. 18ECh. 3 - Prob. 19ECh. 3 - Prob. 20ECh. 3 - 17.35 The samples of nitric and acetic acids shows...Ch. 3 - 17.36 Determine whether each of the following...Ch. 3 - Prob. 23ECh. 3 - Prob. 24ECh. 3 - Prob. 25ECh. 3 - Assume that 30.0 mL of a M solution of a week base...Ch. 3 - Prob. 27ECh. 3 - Prob. 28ECh. 3 - Prob. 29ECh. 3 - Prob. 30ECh. 3 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 3 - Prob. 32ECh. 3 - Prob. 33ECh. 3 - Prob. 34ECh. 3 - The solubility of two slighty soluble salts of...Ch. 3 - Prob. 36ECh. 3 - 17.52
a. true or false: solubility and...Ch. 3 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 3 - Prob. 39ECh. 3 - Prob. 40ECh. 3 - using calculate the molar solubility of AgBr in a....Ch. 3 - calculate the solubility of LaF3 in grams per...Ch. 3 - Prob. 43ECh. 3 - Consider a beaker containing a saturated solution...Ch. 3 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 3 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 3 - 17.63 Which of the following salts will be...Ch. 3 - For each of the following slightly soluble salts,...Ch. 3 - Prob. 49ECh. 3 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 3 - Prob. 51ECh. 3 - Prob. 52ECh. 3 - Prob. 53ECh. 3 - Calculate the minimum pH needed to precipitate Mn...Ch. 3 - Prob. 55ECh. 3 - Prob. 56ECh. 3 - Prob. 57ECh. 3 - Prob. 58ECh. 3 - Prob. 59ECh. 3 - An unknown solid is entirely soluble in water. On...Ch. 3 - Prob. 61ECh. 3 - Prob. 62ECh. 3 - 17.81
Precipitation of the group 4 cautions of...Ch. 3 - Prob. 64ECh. 3 - Prob. 65ECh. 3 - Prob. 66ECh. 3 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 3 - Prob. 68ECh. 3 - Equal quantities of 0.010 M solution of an acid HA...Ch. 3 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 3 - (a) Define the terms limiting reactant and excess...Ch. 3 - Prob. 72ECh. 3 - Prob. 73ECh. 3 - Prob. 74ECh. 3 - What is the pH of a solution made by mixing 0.30...Ch. 3 - Suppose you want to do a physiological experiment...Ch. 3 - Prob. 77ECh. 3 - Prob. 78ECh. 3 - For each pair of compounds, use Kap values to...Ch. 3 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 3 - Salts containing the phosphate ion are added to...Ch. 3 - Prob. 82ECh. 3 - 17.103 The solubility –product constant for barium...Ch. 3 - Prob. 84ECh. 3 - Prob. 85ECh. 3 - A buffer of what pH is needed to give a Mg2+...Ch. 3 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 3 - Prob. 88AECh. 3 - Prob. 89AECh. 3 - Prob. 90AECh. 3 - Prob. 91AECh. 3 - Prob. 92AECh. 3 - Prob. 93AECh. 3 - Prob. 94AECh. 3 - Prob. 95AECh. 3 - A concentration of 10-100 parts per billion (by...Ch. 3 - Prob. 97AECh. 3 - Prob. 98AECh. 3 - In nonaqueous solvents, it is possible to react HF...Ch. 3 - Prob. 100AECh. 3 - Prob. 101AECh. 3 - Prob. 102AECh. 3 - 17.9 The following graphs represent the behavior...Ch. 3 - Prob. 104AECh. 3 - 17.11 The graph below shows the solubility of a...Ch. 3 - Prob. 106IECh. 3 - Prob. 107IECh. 3 - (a) If an automobile travels 225 mi with a gas...Ch. 3 - Prob. 109IECh. 3 - Prob. 110IECh. 3 - Hydrogen cyanide, HCN, is a poisonous gas. The...Ch. 3 - Prob. 112IE
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Consider the following beakers. Each contains a solution of the hypothetical atom X. a Arrange the beakers in order of increasing concentration of X. b Without adding or removing X, what specific things could you do to make the concentrations of X equal in each beaker? (Hint: Think about dilutions.)arrow_forwardA 0.010 M solution of ammonia, NH3, has a pH of 10.6 at 25C. What is the concentration of hydroxide ion? (One way to solve this problem is to find the pOH first and then calculate the hydroxide-ion concentration.)arrow_forwardWhich of the following would you expect to be strong electrolytes when placed in water? NH4ClMgBr2H2OHClCa3(PO4)2CH3OH Which of the statements below support the answers you chose above? (Pick as many as apply.) a Ionic compounds always produce a significant number of ions in aqueous solution. b A molecular compound can be either a weak electrolyte or a nonelectrolyte. c Soluble ionic compounds are strong electrolytes. d Water conducts electricity so that whenever water is present, we would expect a strong electrolyte. e Some molecular substances completely ionize in aqueous solution.arrow_forward
- What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)? (Answer is not 11.16)arrow_forwardConsider three flasks, each containing 0.10 mol of acid. You need to learn something about the acids in each of the flasks, so you perform titration using a NaOH solution. Here are the results of the experiment: Flask A 10 mL of NaOH required for neutralization Flask B 20 mL of NaOH required for neutralization Flask C 30 mL of NaOH required for neutralization a What have you learned about each of these acids from performing the experiment? b Could you use the results of this experiment to determine the concentration of the NaOH? If not, what assumption about the molecular formulas of the acids would allow you to make the concentration determination?arrow_forwardWhich member of each of the following pairs is the stranger acid? a. NH3, PH3; b. HI, H2Te; c. HSO3, H2SO3; d. H3AsO4, H3AsO3; e. HSO4, HSeO4arrow_forward
- Quinine is an alkaloid, or naturally occurring base, used to treat malaria. A 0.0015 M solution of quinine has a pH of 9.84. The basicity of alkaloids is due to a nitrogen atom that picks up protons from water in the same manner as ammonia does. What is Kb?arrow_forwardThe chemical equation for the hydrolysis of nitrous acid is HNO2(aq)+H2O(l)H3O+(aq)+NO2(aq) Which of the following, when added to a nitrous acid solution, would reduce the degree of ionization of the acid: NaNO3 (aq), KNO2(aq), HNO3(aq), or NaCl(aq)?arrow_forwardExercise 16.2 Calculate [H+] in a solution in which [OH]=2.0102M. Is this solution acidic, neutral, or basic?arrow_forward
- EXERCISE 5: ACIDS AND BASES Tell whether each of the following statements is characteristic of an acid or a Neutralizes acids Has a soapy feel Neutralizes bases Turns litmus to red Identify the acid and base on the left side of the following equations and identify their conjugate species on the right 3 (aq) H2CO3 (aq) + H2O (l) H3O+ (aq) + HCO - NH4 + (aq) + H2O (l) H3O+ (aq) + NH3 (aq) 2 (aq) 2 (aq) HCN (aq) + NO - CN- (aq) + HNO - Equation Acid Base Conjugate base Conjugate acid 1 2 3 Complete…arrow_forwardProblem 6-9 Sodium hydrogen sulfate, NaHSO4, which dissolves in water to release H+ ion, is used to adjust the pH of the water in swimming pools. Suppose we add 560. g of NaHSO4 to a swimming pool that contains L of water at 25°C. What is the Na+ ion concentration in ppm?arrow_forwardYou have prepared dilute solutions of equal molar concentrations of HC2H3O2 (acetic arid), HNO2, HF, and HCN. Rank the solutions from the highest pH to the lowest pH. (Refer to Table 16.1.)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY