Here are a couple questions I can\'t seem to figure out, help is needed thank yo

Question

Here are a couple questions I can't seem to figure out, help is needed thank you!

1. For each pair, will a solution of both be a buffer solution? Why or why not?

A) Sulfuric acid and sodium sulfate

B) HClO2 and NaClO2

C) Hydroiodic acid and calcium iodide

D) HBrO and potassium hypobromate

E) HBr and sodium bromate

2. A) For each pair of reactants, balance the neutralization reaction (all materials in aqueous solution). Label each Bronsted-Lowry Acid, Base, Conjugate Acid, Conjugate Base.

OH-1(aq) + HCl9aq) <----> ___________

NH3(aq) + HCH3CO2(aq) <----> _____________

B) Identify four Lewis bases from problem 2 and explain why they are lewis bases.

3. A) If a buffer solution is made from .015 moles of a weak acid like Acetic acid and .010 moles of sodium acetate in a liter of water, how many moles of strong base will destroy the buffering ability of this solution?

B) How many moles of strong acid will destroy the buffering ability of this solution?

Thank you so much!!!

Explanation / Answer

1)B) HClO2 and NaClO2

D) HBrO and potassium hypobromate

buffer solution is formed by salts of weak acid or bases woith the acid or bases

2)HCl + OH- --> H2O + Cl- (all in aq)

acid-HCl

base-OH-

conj.acid --> H2O

conj. base= Cl-

NH3 + CH3COOH --> CH3COO- + NH4+ (all in aq)

acid-CH3COOH

base- NH3

conj. acid---> NH4+

conj. base ---> CH3COO-

B)lewis bases donate a pair of electrons .

so they are OH- , Cl- , NH3 , CH3COO-

3)A) 0.015 moles of a base will neutralise the acid present and will destroy the buffer.

B)0.01 moles of a strong acid will neutralise the acetate salt and hence destroy the buffer

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