How many milliliters of a stock solution of 6.0 M HNO3 would be required to prepare 110 mL of 0.500 M HNO3 solution?
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To find out how many milliliters of the stock solution are required, we can use the equation:
M1V1 = M2V2
where M1 is the molarity of the stock solution, V1 is the volume of the stock solution, M2 is the desired molarity of the final solution, and V2 is the desired volume of the final solution.
In this case, the molarity of the stock solution is 6.0 M, the desired molarity of the final solution is 0.500 M, and the desired volume of the final solution is 110 mL.
Plugging these values into the equation:
(6.0 M)(V1) = (0.500 M)(110 mL)
Simplifying:
6.0 V1 = 0.500 * 110
6.0 V1 = 55
Dividing both sides by 6:
V1 = 55 / 6
V1 = approximately 9.17 mL
Therefore, approximately 9.17 milliliters of the stock solution are required to prepare 110 mL of 0.500 M HNO3 solution.
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