What is the molarity of NaCl when 3.46 g of NaCl is dissolved in water to form 50.0 mL of solution?

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What is the molarity of NaCl when 3.46 g of NaCl is dissolved in water to form 50.0 mL of solution?

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Answer 1 · 2018-01-15T05:14:03

$[N a C l (a q)] = \cdot m o l \cdot L^{- 1} ≅ 1.20 \cdot m o l \cdot L^{- 1}$ $[NaCl(aq)]=*mol*L^-1~=1.20*mol*L^-1$ ..

Explanation:

For $molarity$ $"molarity"$ we take the quotient... $\frac{moles of solute}{volume of solution}$ $"moles of solute"/"volume of solution"$ ...and we get an answer with units of $m o l \cdot L^{- 1}$ $mol*L^-1$ ..

And so.... $\frac{\frac{3.46 \cdot g}{58.44 \cdot g \cdot m o l^{- 1}}}{50.0 \cdot m L \times 10^{- 3} \cdot L \cdot m L^{- 1}} = ? ? \cdot m o l \cdot L^{- 1}$ $((3.46*g)/(58.44*g*mol^-1))/(50.0*mLxx10^-3*L*mL^-1)=??*mol*L^-1$ ...

What are the values of $[N a^{+}]$ $[Na^+]$ and $[C l^{-}]$ $[Cl^-]$ ?

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What is the molarity of NaCl when 3.46 g of NaCl is dissolved in water to form 50.0 mL of solution?

1 Answer

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