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Alexus [3.1K]
2 years ago
13

29.47 mL of a solution of the acid HBr is titrated, and 72.90 mL of 0.2500-M NaOH is required to reach the equivalence point. Ca

lculate the original concentration of the acid solution.
Chemistry
1 answer:
Klio2033 [76]2 years ago
4 0

The original concentration of the acid solution is 6.175 \times 10^-4 mol / L.

<u>Explanation:</u>

Concentration is the ratio of solute in a solution to either solvent or total solution. It is expressed in terms of mass per unit volume

                        HBr + NaOH -----> NaBr + H2O

There is a 1:1 equivalence with acid and base.

Moles of NaOH = 72.90 \times 10^-3 \times 0.25

                          = 0.0182 mol.

[ HBr ] = moles of base / volume of a solution

          = 0.0182 / 29.47

          = 6.175 \times 10^-4 mol / L.

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What is the ph of a solution that has a [h ] = 0. 0039 m?
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5 0
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Question 5
baherus [9]

Answer:

2.03 atm

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3 years ago
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