Homework Answers
9) When a weak acid and strong base is mixed then the resulting pH will be > 7 because weak acid dissociate partially and strong base dissociate completely thus make the Solution more basic.
10) Lewis base are electron pair donors.
11) Higher electronegativity of A in H-A increase the acid strength. Because of high electronegativity of A it Increase the positive charge on H and make it more acidic.
12) Larger size of A in H-A increase the acid strength of HA. Because H-A bond become weaker and it become easy to release proton.
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0 TOXO 9. When a weak acid and a strong base are mixed, the resulting pH...
just answer please 10. For Lewis acids and bases, the base is defined as an electron...
just answer please
10. For Lewis acids and bases, the base is defined as an electron pair donor/acceptor (circle the correct answer). 11. When comparing anions from the same period, higher electronegativity of A in the H-A bond increases / decreases (circle the correct answer) acid strength 12. When comparing anions from the same group, larger size of A in the H A bond Increases / decreases (circle the correct answer) acid strength 13. A 0.10 M solution of a...
This reaction is classified as: Strong Acid + Strong Base, Weak Acid + Strong Base, Strong Acid + Weak Base, Weak Aci...
This reaction is classified as: Strong Acid + Strong Base, Weak
Acid + Strong Base, Strong Acid + Weak Base, Weak Acid + Weak
Base.
The extent of this reaction is: Below 50%, 50%, Above 50%,
100%
When 35.0 mL of 0.300 M
perchloric acid and 35.0 mL of
0.150 M barium hypochlorite are
combined, the pH of the resulting solution will be greater than,
equal to, less than seven.
Write the balanced NET IONIC equation for the reaction that...
When a weak acid is titrated with a strong base, if the pH at the half-equivalence...
When a weak acid is titrated with a strong base, if the pH at the half-equivalence point is 6.04, what is the Ka of the acid?
9. Classify each substance as a strong acid (SA), weak acid (WA), strong base (SB), or...
9. Classify each substance as a strong acid (SA), weak acid (WA), strong base (SB), or weak base (WB). Then calculate the pH and % ionization. a. 1.0 M HC,H,O, d. 0.01 M HC,H,O b. 0.25 M HC,H,O c. 0.1 M HC,H,0,
9. Classify each substance as a strong acid (SA), weak acid (WA), strong base (SB), or weak base (WB). Then calculate the pH and % ionization. a. 1.0 M HC,H,O, d. 0.01 M HC,H,O b. 0.25 M HC,H,O...
1. a. Draw the pH curve for a strong acid and a weak acid when a...
1. a. Draw the pH curve for a strong acid and a weak acid when a strong base is added. Note the in the case of the weak acid, the addition of the strong base yields a common ion (i.e conjugate base) when it is dissolved. b. Explain the difference between the two curves. (Hint: why is one curve showing a very small change in pH along y-axis in the acidic region when the strong base is added?
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base...
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
Classify H_2CO_3 as a strong base, weak base, strong acid, or weak acid, and then answer...
Classify H_2CO_3 as a strong base, weak base, strong acid, or weak acid, and then answer the following question. What is the pH of a 0.321 M H_2CO_3(aq) solution? 3.4 8.6 5.4 10.6 6.9
1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write...
1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write the neutralization reaction for HF and KOH. What is the value of Kn (equilibrium constant for neutralization)? (Ka(HF)=3.5*10^-4). If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic, or neutral? Answer: Kn= 3.5*10^10; neutralization reaction is 100% complete since Kn is so large; pH > 7 at equivalence. Just need this explained please :)
Classify HCIO as a strong base, weak base, strong acid, or weak acid, and then answer...
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...
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
just answer please
10. For Lewis acids and bases, the base is defined as an electron pair donor/acceptor (circle the correct answer). 11. When comparing anions from the same period, higher electronegativity of A in the H-A bond increases / decreases (circle the correct answer) acid strength 12. When comparing anions from the same group, larger size of A in the H A bond Increases / decreases (circle the correct answer) acid strength 13. A 0.10 M solution of a...
This reaction is classified as: Strong Acid + Strong Base, Weak
Acid + Strong Base, Strong Acid + Weak Base, Weak Acid + Weak
Base.
The extent of this reaction is: Below 50%, 50%, Above 50%,
100%
When 35.0 mL of 0.300 M
perchloric acid and 35.0 mL of
0.150 M barium hypochlorite are
combined, the pH of the resulting solution will be greater than,
equal to, less than seven.
Write the balanced NET IONIC equation for the reaction that...
9. Classify each substance as a strong acid (SA), weak acid (WA), strong base (SB), or weak base (WB). Then calculate the pH and % ionization. a. 1.0 M HC,H,O, d. 0.01 M HC,H,O b. 0.25 M HC,H,O c. 0.1 M HC,H,0,
9. Classify each substance as a strong acid (SA), weak acid (WA), strong base (SB), or weak base (WB). Then calculate the pH and % ionization. a. 1.0 M HC,H,O, d. 0.01 M HC,H,O b. 0.25 M HC,H,O...
1. a. Draw the pH curve for a strong acid and a weak acid when a strong base is added. Note the in the case of the weak acid, the addition of the strong base yields a common ion (i.e conjugate base) when it is dissolved. b. Explain the difference between the two curves. (Hint: why is one curve showing a very small change in pH along y-axis in the acidic region when the strong base is added?
Classify H_2CO_3 as a strong base, weak base, strong acid, or weak acid, and then answer the following question. What is the pH of a 0.321 M H_2CO_3(aq) solution? 3.4 8.6 5.4 10.6 6.9
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
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