Question 1 (1 point) If 10 mL of 0.100 M NaOH was needed to neutralize 50 mL of

ID: 1060200 • Letter: Q

Question

Question 1 (1 point)

If 10 mL of 0.100 M NaOH was needed to neutralize 50 mL of a KHSO4 solution, how many moles of the KHSO4 was present?

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Question 2 (1 point)

Phenolphthalein turns ______ when the equivalence point is reached for your acid-base titration and as excess NaOH is added.

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red

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Question 3 (1 point)

What volume (in mL) of 0.1 M NaOH would be needed to neutralize 50 mL of 0.1 M diprotic acid, H2SO4?

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Question 4 (1 point)

If, after the addition of phenolphthalein, your titration solution turned dark pink during the titration that meant __________.

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Question 5 (1 point)

Phenolphthalein is an example of an ___________, which are used to determine the acidity or alkalinity of a solution via color.

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a) 0.005 mol KHSO4 b) 0.05 mol KHSO4 c) 0.02 mol KHSO4 d) 0.001 mol KHSO4

1) NaOH + KHSO4 -------------> H2O + NaKSO4

millimoles of NaOH = 10 x 0.1 = 1.0

moles of NaOH = 1.0 / 1000 = 0.001 moles

both are reacting 1 : 1 ratio so 0.001 moles KHSo4 must be present

answer = option d = 0.001 moles of KHSO4

2) answer = option d = pink

3) answer = option b = 100 mL

4) answer = option a = You added too much NaOH and went too far past the equivalence point.