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16 Nov 2019

8.8 mL of 3.0 M acetic acid added to beaker containing 3.578g of sodium acetate. 55.6 mL of water added to that solution. What is the theoretical pH of this buffer solution?

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Hubert Koch
Hubert KochLv2
19 Sep 2019

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Related questions

a) How to do I calculate the pH of original buffer given mass ofNaC2H3O2*H2O (FW =136 g/mol) = 3.507 g
after measuring out 8.8 mL of 3.0 M acetic acid to add to thebeaker containing the sodium acetate. Then put in 55.6 mL ofdistilled water with the pH of original buffer solution =4.89

b) How then, how would I calculate the pH of a buffer + NCl aftertaking 32 mL of the solution noted above and pipet 1.0 mL of 6.0 MHCl with the pH of buffer + HCl = 4.41?

c) Finally, how to calculate the pH of buffer + NaOH with 32 mL ofthe first solution listed above and pipet 1.0 mL of 6.0 M NaOH withpH of buffer + NaOH = 5.28?

I need help on this problem please!!

3.490 g of NaC2H3O2*3H2O, 8.8 ml of acetic acid was added then 55.6 ml of distilled water was added too, and ph was measured and it was found to be 4.7

Then half of the buffer was poured into another beaker and labeled beaker 1 and 2

1.0ml of 6.0M HCL was was added into beaker 1 and ph was found to be 4.2

1.0 ml of 6.0 NaOH into beaker 2 and ph was found to be 5.0

1) calculate the ph of original buffer (use ICE box method )

2)calculate the ph of buffer + HCl (use ICE box method )

3) calculate the ph of buffer + NaOH (use ICE box method )

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