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silviamgarcia
24.07.2019 •
Chemistry
You have two 466.0 ml aqueous solutions. solution a is a solution of silver nitrate, and solution b is a solution of potassium chromate. the masses of the solutes in each of the solutions are the same. when the solutions are added together, a blood-red precipitate forms. after the reaction has gone to completion, you dry the solid and find that it has a mass of 331.8 g. (a) calculate the concentration of the potassium ions in the original potassium chromate solution.(b) calculate the concentration of the chromate ions in the final solution
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Ответ:
The concentration of the potassium ions in the original potassium chromate solution is 4.2927 mol/L.
The concentration of the chromate ions in the final solution is 1.0731 mol/L.
Explanation:
Volume of solution A i.e. solution of silver nitrate = 466.0 mL = 0.466 L
Volume of solution B i.e. solution of potassium chromate = 466.0 mL = 0.466 L
Moles of silver chromate =![\frac{331.8}{331.73 g/mol}=1.0002 mol](/tpl/images/0127/0717/6df31.png)
According to reaction , 1 mol of silver chromate is produce from 2 moles of silver nitrate.
Then, 1.0002 moles of silver chromate will be formed from:
According to reaction , 1 mol of silver chromate is produce from 1 mole of potassium chromate.
Then, 1.0002 moles of silver chromate will be formed from:
a) The concentration of the potassium ions in the original potassium chromate solution.
Volume of the original solution = 0.466 L
1 mol of potassium chromate dissociates into 2mol of potassium ions and 1 mol of chromate ions:
Moles of potassium ions = 2 × 1.0002 mol = 2.0004 mol
b) The concentration of the chromate ions in the final solution
Volume of the final solution = 0.466 L + 0.466 L
Moles of chromate ions = 1 × 1.0002 mol = 1.0002 mol
Ответ:
Answer
I dont know
Explanation:
do it yourself