Question

In: Chemistry

calculate pH from 75 ml of 0.1M CH3COOH and 25 ml of 0.1 M Ca(OH)2

Expert Solution

a.) pH from 75 mL of 0.1M CH3COOH

0.1M.......................................... 0............................0

-x ............................................... x ...........................x

(0.1-x)....................................... x .......................... x

pH is determined by -log[H₃O]⁺

b. pH of 25mL of 0.1 M Ca(OH)₂

Concentration OH^-= 2*0.1= 0.2 M

pOH= -log [OH] = -log [0.2]= 0.70

pH=14-0.70= 13.3

c. Neutralization

moles CH3COOH= 75x10^-3 L* 0.1M=7.5x10^-3 moles

moles Ca(OH)₂= 25 x10^-3 L* 0.1 M= 2.5x 10^-3 moles

7.5 x 10^-3 moles.........2.5x 10^-3 moles

-2(2.5x 10^-3 moles)..... -2.5x 10^-3 moles.......... 2.5x 10^-3 moles..... 2.5x 10^-3 moles

2.5x 10^-3 moles............0..................................2.5x 10^-3 moles.........2.5x 10^-3 moles

pH is determined by the Henderson Hasselbach equation

queen_honey_blossom answered 2 hours ago

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