A 100.0 mL sample of0.200 M acetic acid (K a = 1.8 * 10 -5 ) istitrated with 100
ID: 682777 • Letter: A
Question
A 100.0 mL sample of0.200 M acetic acid (Ka = 1.8 * 10-5) istitrated with 100 mL of 0.200 M NaOH. What is thepH? I'm so confused about this because they're being titrated tothe equivalence point. Because it's a weak acid/strong base I know the pH will be above 7but I don't know how to do this problem... CH3COOH + OH ---> CH3COO- +H2O I 0.1 M 0.1M 0 N/A C -0.1 -0.1 +0.1 N/A E0 0 0.1 N/A Normally if I had OH left over I'd use it to find the pH andif I had CH3COOH I'd use a second ICE diagram to findthe pH but because I have nothing left of either I don't know what to donext... A 100.0 mL sample of0.200 M acetic acid (Ka = 1.8 * 10-5) istitrated with 100 mL of 0.200 M NaOH. What is thepH? I'm so confused about this because they're being titrated tothe equivalence point. Because it's a weak acid/strong base I know the pH will be above 7but I don't know how to do this problem... CH3COOH + OH ---> CH3COO- +H2O I 0.1 M 0.1M 0 N/A C -0.1 -0.1 +0.1 N/A E0 0 0.1 N/A Normally if I had OH left over I'd use it to find the pH andif I had CH3COOH I'd use a second ICE diagram to findthe pH but because I have nothing left of either I don't know what to donext... CH3COOH + OH ---> CH3COO- +H2O I 0.1 M 0.1M 0 N/A C -0.1 -0.1 +0.1 N/A E0 0 0.1 N/A Normally if I had OH left over I'd use it to find the pH andif I had CH3COOH I'd use a second ICE diagram to findthe pH but because I have nothing left of either I don't know what to donext...Explanation / Answer
your ice table needs to contain values in units of moles... for example Acetic Acid I = .200 M x .1L = .02moles
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