a. What is the concentration of H* in 0.030M HNO,? b. What is the pH of the solution? c. What is the OH concentration in the solution? d. What is the pOH of the soluțion? 3. Complete the following: 129 words English (United States) Focus 3. Complete the following: [H*] [ОН] pH РОН Acidity 1.8 x 10-6 M 3.6 x 10-10 M 8.15 Spring 2020 5.70 Page 1 of 2. 129 words Engiish (Unted States) O Focus Boo

a. What is the concentration of H* in 0.030M HNO,? b. What is the pH of the solution? c. What is the OH concentration in the solution? d. What is the pOH of the soluțion? 3. Complete the following: 129 words English (United States) Focus 3. Complete the following: [H*] [ОН] pH РОН Acidity 1.8 x 10-6 M 3.6 x 10-10 M 8.15 Spring 2020 5.70 Page 1 of 2. 129 words Engiish (Unted States) O Focus Boo

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter25: Ph Measurements-buffers And Their Properties

Section: Chapter Questions

Problem 3ASA: The pH of a 0.10 MHOBr solution is 4.8. What is H in that solution? ____________M What is OBr-? What...

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Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in Table 13-3. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?
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The pH of a 0.10 MHOBr solution is 4.8. What is H in that solution? ____________M What is OBr-? What is HOBr? Where do the H and OBr- ions comes from? ____________M; ____________M What is the value of Ka for HOBr? What is the value of pKa?____________ ____________
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.
Blood is buffered mainly by the HCO3 H2CO3 buffer system. The normal pH of blood is 7.40. (a) Calculate the [ H2CO3 ]/[ HCO3 ] ratio. (b) What does the pH become if 15% of the HCO3 ions are converted toH2CO3? (c) What does the pH become if 15% of the H2CO3 molecules converted to HCO3 ions?
A solution of KOH has a pH of 13.29. It requires 27.66 mL of 0.2500 M HCI to reach the equivalence point. (a) What is the volume of the KOH solution? (b) What is the pH at the equivalence point? (c) What is [K+] and [Cl-] at the equivalence point? Assume volumes are additive.
. For each hydrogen or hydroxide ion concentration listed. calculate the concentration of the complementary ion and the pH and pOH of the solution. a. [H+]=5.72104M b. [OH-]=8.91105Mc. [H+]=2.871012Md. [OH-]=7.22108M
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.