What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution?

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What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution?

chemistry molarity

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Answer 1 · 2018-02-19T18:53:06

Molarity = $0.154$ $0.154$ $M$ $M$

Explanation:

mass of $K C l$ $KCl$ = $4.88$ $4.88$ $g$ $g$
molar mass of $K C l$ $KCl$ = $74.55$ $74.55$ $g$ $g$ / $m o l$ $mol$
no. of moles = $4.88$ $4.88$ g/ $74.55$ $74.55$ $g$ $g$ / $m o l$ $mol$ = $0.0654$ $0.0654$ moles
volume of solution = $423 m l$ $423 ml$ = $0.423 L$ $0.423L$
Molarity = no. of moles/volume of solution
Molarity = $0.0654$ $0.0654$ moles/ $0.423 L$ $0.423L$
Molarity = $0.154$ $0.154$ $M$ $M$

Answer 2 · 2018-02-19T18:54:48

We take the quotient... $molarity = \frac{moles of solute}{volume of solution}$ $"molarity"="moles of solute"/"volume of solution"$

Explanation:

Here........... $"Molarity"=(underbrace((4.88*g)/(74.55*g*mol^-1))_"moles of solute")/underbrace(423*mLxx10^-3L*mL^-1)_"volume of solution"=0.155*mol*L^-1$

And note that the quotient automatically gives the units required for $"concentration".$

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What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution?

chemistry molarity

2 Answers

Explanation:

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