LINO3 is added to water. Will it change the pH, and if so, how? Yes, and the pH will be < 7 impossible to tell No, the pH will remain unchanged. O Yes, and the pH will be > 7. You want an aqueous solution to be more basic. Choose the correct salt below that would accomplish this. O NH4NO3 O NazPO4 Caz(PO4)2 O none of these salts will cause the pH to increase

LINO3 is added to water. Will it change the pH, and if so, how? Yes, and the pH will be < 7 impossible to tell No, the pH will remain unchanged. O Yes, and the pH will be > 7. You want an aqueous solution to be more basic. Choose the correct salt below that would accomplish this. O NH4NO3 O NazPO4 Caz(PO4)2 O none of these salts will cause the pH to increase

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 19QAP: . How is the strength of an acid related to the fact that a competition for protons exists in...

See similar textbooks

Similar questions

You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
Consider a salt of a weak base and a weak acid such as ammonium cyanide. Both the NH4+ and CN ions interact with water in aqueous solution, but the net reaction can be considered as a proton transfer from NH4+ to CN. NH4+(aq) + CN(aq) NH3(aq) + HCN(aq) (a) Show that the equilibrium constant for this reaction, Kact, is 1. Knet=KaKbKw where Ka is the ionization constant for the weak acid NH4+ and Kb, is the constant for the weak base CN. (b) Calculate Knet values fur each of the following, NH4CN, NH4CH3CO2, and NH4K Which salt has the largest value of Kact, and why? (c) Predict whether a solution of each of the compounds in (b) is acidic or basic. Explain how you made this prediction (Yon do not need a calculation to make this prediction.)
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
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.
Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. Use 1.80105 as Ka for acetic acid. (a) What is the pH of the solution? (b) Is the solution acidic or basic? (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of the original buffer?
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?