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23 Nov 2019

In an acid-base titration, 26.81 mL of a NaOH solution are needed to neutralize 26.98 mL of a 0.1490 M HCl solution. Find the molarity of the NaOH solution.

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Beverley Smith
Beverley SmithLv2
5 Jul 2019

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Related questions

In an acid-base titration, 24.88 mL of an NaOH solution are needed to neutralize 26.43 mL of a 0.1049 M HCl solution, To find the molarity of the NaOH solution, we can use the following procedure: a First note the value of MH- in the HCl solution. b. Find MOH- in the NaOH solution. c. Obtain MNaOH from MOH-.

A solution of malonic acid was standardized by titration with 0.100 M NaOH solution. If 20.76 mL of the NaOH solution were required to neutralize completely 13.15 mL of malonic acid solution, what is the molarity of the malonic acid solution?

This is the question above:

In an acid-base titration, 22.13 mL of a NaOH solution are needed to neutralize 24.65 mL of the potassium hydrogen phthalate solution, which was prepared in Question #1. Determine the molarity of the NaOH solution. Start with a balanced equation.

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This is the question needing answering:

0.001081

Using the above sodium hydroxide solution, 27.21 mL of the NaOH solution is required to neutralize a volume of 28.45 mL of an acetic acid solution having an unknown concentration to a phenolphthalein end point. Determine the concentration, in molarity, of the acidic solution. Start with a balanced equation. 0.04884 0.01256 0.001329 0.05024 0.04671 0.4384

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