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calculate the ph of 20 ml of .1M NaOH to 40 ml of acetic acid
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I did an experiment using 20ml of 0.1M acetic acid and added 8ml of 0.1M NaOH. pH obtained after adding NaOH was 5.2. How do i
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To save some typing, I will call acetic acid, HAc and acetate is Ac^- millimoles HAc = mL x M = 20 x
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What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid,
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The equation is CH3COOH + NaOH ==> CH3COONa + H2O (What you wrote--C6H5COOH-- is benzoic acid). I
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Please help me... I don't understand this at all. I need to calculate the molarity of the acetic acid in this problem:
A 4,00 mL
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So far so good; however, you didn't include the volume of NaOH required in the titration. M(NaOH) x
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19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of
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19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L
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Calculate the amount (in mL) of 1.520M NaOH that is required to add the following acetic acid solution to prepare a buffer with
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You had this in math. It isn't chemistry. 5.75 = 4.74 + log b/a 1.01 = log b/a 10^(b/a) = 1.01 Plug
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Calculate the amount (in mL) of 1.520M NaOH that is required to add the following acetic acid solution to prepare a buffer with
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I would do this. 5% w/v means 5g HAc/100 mL solution which is (5/60) mols/100 and that is 5/60/0.1L
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Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH.
a) Calculate
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I agree with your answer of 3.88 for part A (but I don't know that you worked it correctly since you
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Prepare 500mL of a 0.200 M acetate buffer at pH 4.90 using only pure acetic acid, 3M NaOH, and water.
1) Add acetic acid to
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To answer the first question and determine the amount of acetic acid needed, we need to use the
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Calculate the percentage of acetic acid used in 2.1g of acetic acid that was titrated against 0.1M NaOH
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To calculate the percentage of acetic acid in 2.1g of acetic acid, we need to know the molecular
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A total of 31.3 ml of 0.15 N NaOH was required to reach a phenolphthalein endpoint in titrating 6.00 g vinegar. Calculate the
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Liters x normality x equivalent weight = grams. I prefer to use mL x N x milliequivalent weight =
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