Macmillan The quality assurance lab just received a shipment of three solutions. The lab manager asks you to verify the stock solutions and label each bottle with the solution's hydrogen ion concentration, [H+]. You first use the pH meter to determine the pH of each solution. Calculate the hydrogen ion concentration of solution #1, which has pH 2.50. Calculate the hydrogen ion concentration of solution #2, which has pH 5.50. [H+] = 0.00316 [H+]= 0.000003 M Incorrect Calculate the hydrogen ion concentration of solution #3, which has pH 12.25. [H+] = 5.62 x10-13 M M

Macmillan The quality assurance lab just received a shipment of three solutions. The lab manager asks you to verify the stock solutions and label each bottle with the solution's hydrogen ion concentration, [H+]. You first use the pH meter to determine the pH of each solution. Calculate the hydrogen ion concentration of solution #1, which has pH 2.50. Calculate the hydrogen ion concentration of solution #2, which has pH 5.50. [H+] = 0.00316 [H+]= 0.000003 M Incorrect Calculate the hydrogen ion concentration of solution #3, which has pH 12.25. [H+] = 5.62 x10-13 M M

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

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ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

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Problem 6E

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Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Indicate whether each of the following samples is acidic, basic, or neutral. a. butter, pH 6.1 b. lemon juice, pH 2.2 c. peach, pH 3.5 d. milk of magnesia, pH 10.5
Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Use the same symbols as in Question 61 ( = anion, =OH) for the box below. (a) Fill in a similar box (representing one liter of the same solution) after 2 mol of H+ (2) have been added. Indicate whether the resulting solution is an acid, base, or buffer. (b) Follow the directions of part (a) for the resulting solution after 2 mol of OH- (2 ) have been added. (c) Follow the directions of part (a) for the resulting solution after 5 mol of OH- (5 ) have been added. (Hint: Write the equation for the reaction before you draw the results.)
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
A sample of coffee has a pH of 4.3. Calculate the hydronium ion concentration in this coffee. Is the coffee acidic or basic?
Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000?

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