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

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter14: Acid-base Equilibria

Section: Chapter Questions

Problem 48E: Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in...

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For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
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.
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 0.10 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?____________ ____________
Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution of HNO3(d=1.00g/mL). What is the pH of 10.0 mL of the same sample? (b) A solution made up of 1.0 g of HCI dissolved in enough water to make 1.28 L of solution. What is the pH of the solution? If the same mass of HCI is dissolved in enough water to make 128 mL of solution, what would the pH be?
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.
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
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?
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?
Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? Explain your answer.
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?
Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.