answer

watching

views

13 Dec 2019

Which of these are either strong, weak or non-electrolytes?Warm tap water:0,9 % NaCl (aq): 1% sucrose solution:Glacial acetic acid:0,1 M acetic acid:40% ethanol:0,1 M HCl:0,1 M NaC2H3O2 (aq):0,1 M ammonia:And If they are either strong or weak, what ions are there in the solution?

answer

watching

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Casey DurganLv2

17 Dec 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Please arrange the following acids in order of increasing strength.

H3PO4 < H2PO4- < HPO4 ^-2

H2PO4- < H3PO4 < HPO4 ^-2

HPO4-2 < H2PO4- < H3PO4

H3PO4 < HPO4 ^-2 < H2PO4-

All of these acids have the same strength

Consider the following Ka values;

acetic acid Ka[CH3COOH (aq)] = 1.80 x 10^-5

chloroacetic acid Ka[CH2ClCOOH (aq)] = 1.40 x 10^-3

hypochlorous acid Ka[HClO (aq)] = 2.90 x 10^-8

hydrofluoric acid Ka[HF (aq)] = 6.30 x 10^-4

formic acid Ka[HCOOH (aq)] = 1.80 x 10^-4

Which of the following is a correct statement?

Hypochlorous acid is the weakest acid listed

Acetic acid is a weaker acid than hypochlorous acid

Chloroacetic acid is the strongest acid on the list

Formic acid is a stronger acid than acetic acid

Formic acid is a weaker acid than hydrofluoric acid

Which of the following statements strong and weak acids is correct?

Weak acids completely dissociate in solution

Strong acids completely dissociate in solution

A 0.05 M solution of an acid is a weak acid

Strong acids only partially dissociate in solution

Weak acids completely dissociate in solution

Which of the following is not an Arrhenius acid, but is a Lewis acid??

Which of the following compounds is not amphoteric?

a. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution?

b. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with 0.1 M NaOH (aq), at what volume of NaOH (aq) is the equivalence point reached? Is the pH at the equivalence point greater than, less than or the same as in problem #a above? Explain.

c. What is the initial pH expected for a 0.1 M solution of phosphoric acid (H3PO4)? For 25.0 mL of 0.1M H3PO4 (aq), what volume of 0.1 M NaOH (aq) is required to fully titrate all three protons to their end points?

d. In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? How are the pKa and Ka of the weak acid determined from the half equivalence point?

Which of the following statements is(are) true? For the false statements, correct them.

A. A concentrated solution in water will always contain a strong or weak electrolyte.

B. A strong electrolyte will break up into ions when dissolved in water.

C. An acid is a strong electrolyte.

D. All ionic compounds are strong electrolytes in water.