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dangina [55]
3 years ago
12

Complete the following calculations regarding acid/base titrations

Chemistry
1 answer:
madam [21]3 years ago
6 0

Based on the information provided and the assumption that the mole ratio of the acid to the base is 1:1, the molarity of the acid would be 0.0425 M

<h3>Acid/base Titration</h3>

Using the equation:

CaVa = CbVb

This is based on the assumption that the stoichiometric mole ratio of the acid to the base is 1:1.

Ca = CbVb/Va

                   0.1 x 25.5/60 = 0.0425 M

More on acid/base titration can be found here: brainly.com/question/2728613

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if you take 2.0mL of a 7.0 ppm NaOH solution and dilute it to 250.0mL, calculate the final concentration in ppm.
Oduvanchick [21]

Answer:

C₂ = 0.056 ppm

Explanation:

Given data:

Initial volume = 2.0 mL

Initial concentration = 7.0 ppm

Final volume = 250.0 mL

Final concentration = ?

Solution:

Formula:

C₁V₁ = C₂V₂

C₁ = Initial concentration

V₁ = Initial volume

C₂ = Final concentration

V₂ = Final volume

Now we will put the values in formula.

C₁V₁ = C₂V₂

7.0 ppm × 2.0 mL = C₂ × 250.0 mL

C₂ = 14.0 ppm.mL /250.0 mL

C₂ = 0.056 ppm

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