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toricarter00
25.05.2020 •
Chemistry
What is the molarity of a NaOH solution if 15.0 mL is exactly neutralized
by 7.5 mL of a 0.02 M HC2H3O2 solution?
Show all work using titrations formula.
Solved
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Ответ:
see below for explanation
Explanation:
1. you need to set up and balance the equation
NaOH + HC2H3O2 --> NaC2H3O2 + H2O
2. Write the value they gave you underneath the equation to figure out what we are solving for, which is the molarity of NaOH
NaOH (Base) + HC2H3O2 (Acid)--> NaC2H3O2 + H2O
15.0 ml | 7.5ml
? M | 0.02M
3. Use the MaVa=MbVb ·![\frac{mol a}{mol b}](/tpl/images/0665/1043/46381.png)
- This formula is saying the M of an acid times the volume of the acid = the M of the base times the volume of the base times the mol of the acid/ mol of the base ratio. ***You should always compute the volume in Liters.
- Convert your values (x is the molarity of the base, the unknown value) Our acid values are first because that is how the equation is set up
0.0075 · 0.02 = 0.0150 · x · 1/1
4. Simplify
0.00015 = 0.0150x
5. Solve
Molarity of the base = 0.01
Ответ:
Hey mate
after solving the inequality you found option A is correct
thanks