2. Write a NET IONIC equation to show the reaction of HCl with a 3-1 buffer of A

Question

2. Write a NET IONIC equation to show the reaction of HCl with a 3-1 buffer of Acetate to Acetic Acid, Write a similar equation for the reaction of NaOH with the buffer.

3. Twenty drops make about 1 milliliter. Use this to calculate:

a. The pH of a solution after 3 drops 6 M HCl are added to 50 mL H2O.
b. The pH of a solution after 3 drops 6 M HCl are added to 50 mL buffer that has [HAc] = 0.100M and [Ac-] = 0.300M.   

4. Discuss why a relatively insoluble acid will dissolve more easily as it is being titrated (That is - as NaOH is added).

5. Explain why it is not necessary to precisely measure the volume of water that is used to dissolve the solid acid that is to be titrated.

Explanation / Answer

Q2.

Net ionic between HCl and the buffer equation

CH3COOH --> acetic acid, CH3COO- acetate , H+ proton from HCl

there is neutralization of the acetate, and an increase in acid

the ionic equation

CH3COO-(aq) + H+(aq) + Cl-(aq) --> CH3COOH(aq) + Cl-(aq)

Net ionic:

CH3COO-(aq) + H+(aq) --> CH3COOH(aq)

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