We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
QUESTION 38 The conjugate acid of a weak base is a. a weak acid. b. amphiprotic....
When a base accepts a proton it becomes : (a) conjugate base (c) amphiprotic (b) conjugate acid (d) the hydroni um ion The pH of a 10-6M HCl solution 18: (a) 6 (b) 14 (c) 10-8 (d) 8 The titration of a 60.0 ml sample of vinegar required 30.0 ml of 0.60M NaOH, The molarity of the vinegar is: (a) 0.20M (6) 0.30M (c) 0.40M (d) 0.60M The oxidation number of cl in (a) + (c) +6 (b) (d) +5...
A strong acid readily donates a proton, forming a a) Weak conjugate acid c) Strong conjugate base b) Strong conjugate acid d) Weak conjugate base
a buffer is a solution that has a Weak acid in equlibirum with its conjugate base. So can a buffer solution has a weak base in equlibirum with its conjugate acid? So basically, to create a buffer, you can mix a weak acid with its conj. base OR a weak acid + strong base OR a weak base with a strong acid? Am i Correct?
H3PO4 can be classified as a Select one: O a strong acid O b. weak acid O c. strong base O d. weak base NH3 can be classified as a Select one: a strong acid O b. weak acid O c. strong base O d. weak base HNO3 can be classified as a Select one: a strong acid O b. weak acid O c. strong base O d. weak base HCl can be classified as a Select one: O a...
QUESTION 13 Which of the following is false? a. The conjugate base of a relatively weak acid is relatively strong b. Buffer solutions resist changes in pH c. at 25 pH + pOH = 14 d. To make an effective buffer, the pka of the weak acid should be as far away as possible from the pH that you wish to maintain. e. When titrating a weak monoprotic acid with NaOH, at the Veq pt/2, the equation pH pka is...
Question 39 1 pts A weak acid (HA) reacts with a weak base (B) to form the conjugate base of the acid (A) and the conjugate acid of the base (B-H the pKa of HA was 4.8 and the pKa of BH* (i.e., the pKabH of B) was 9.4, what would be the value of the equilibrium constant for the above reaction to the nearest ones? Obviously, by expressing the answer to the nearest ones, we are using too many...
1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a strong acid, weak acid, strong base, or a weak base. Calculate the value of the equilibrium constant II. I. Determine if these reactions need to be treated as an equilibrium (needing an ICE table) or a stoichiometry problem (assuming the reaction goes essentially to completion) a. F-(aq) H2O() HF(aq) + H3O*(aq) + H2O(1) NH3(aq) + b. NH4 (aq) OH (aq) + H3O*(aq) NH3(aq) +...
A weak acid (HA) reacts with a weak base (B) to form the conjugate base of the acid (A-) and the conjugate acid of the base (B-H+). If the pKa of HA was 4.7 and the pKa of BH+ (i.e., the pKabH of B) was 9.4, what would be the value of the equilibrium constant for the above reaction to the nearest ones? Obviously, by expressing the answer to the nearest ones, we are using too many figures than is...
Classify HCIO as a strong base, weak base, strong acid, or weak acid, and then answer the following question. What is the pH of a 0.07 MHCIO (aq) solution? a. 1.2 b.8.7 c. 4.3 d. 9.7 e. 5.3
Classify HCIO as a strong base, weak base, strong acid, or weak acid, and then answer the following question. What is the pH of a 0.07 M HCIO (aq) solution? a. 1.2 b. 8.7 C. 4.3 d. 9.7 e. 5.3