What is the molarity of an $58.5 \cdot g$ $58.5g$ mass of sodium chloride dissolved in enough water to make $1 \cdot L$ $1L$ of solution?

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What is the molarity of an $58.5 \cdot g$ $58.5g$ mass of sodium chloride dissolved in enough water to make $1 \cdot L$ $1L$ of solution?

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Answer 1 · 2016-05-17T17:26:37

$Molarity = \frac{Moles of solute}{Volume of solution}$ $"Molarity "=" Moles of solute"/"Volume of solution"$

Explanation:

If there are $58 \cdot g$ $58*g$ $N a C l$ $NaCl$ solute there are $1$ $1$ $m o l$ $mol$ each solute particles, $N a^{+}$ $Na^+$ , and $C l^{-}$ $Cl^-$ in solution.

And thus $Molarity$ $"Molarity"$ $=$ $=$ $1 \cdot m o l \cdot L^{- 1}$ $1*mol*L^-1$ with respect to $N a C l (a q)$ $NaCl(aq)$ .

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What is the molarity of an $58.5 \cdot g$ $58.5g$ mass of sodium chloride dissolved in enough water to make $1 \cdot L$ $1L$ of solution?

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Explanation:

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What is the molarity of an 58.5⋅g58.5*g mass of sodium chloride dissolved in enough water to make 1⋅L1*L of solution?

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What is the molarity of an $58.5 \cdot g$ $58.5g$ mass of sodium chloride dissolved in enough water to make $1 \cdot L$ $1L$ of solution?