A $60 \cdot m L$ $60mL$ volume of sodium hydroxide at $0.15 \cdot m o l \cdot L^{- 1}$ $0.15molL^-1$ concentration is titrated with $0.500 \cdot m o l \cdot L^{- 1}$ $0.500mol*L^-1$ $H C l (a q)$ $HCl(aq)$ . What volume of acid is required?

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A $60 \cdot m L$ $60mL$ volume of sodium hydroxide at $0.15 \cdot m o l \cdot L^{- 1}$ $0.15molL^-1$ concentration is titrated with $0.500 \cdot m o l \cdot L^{- 1}$ $0.500mol*L^-1$ $H C l (a q)$ $HCl(aq)$ . What volume of acid is required?

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Answer 1 · 2017-05-25T21:49:09

We use the relationship $C_{1} V_{1} = C_{2} V_{2}$ $C_1V_1=C_2V_2$ , where $C_{i}$ $C_i$ , and $V_{i}$ $V_i$ are the individual concentrations/volumes. But FIRST you need a stoichiometric equation. Eventually I gets under $20 \cdot m L$ $20*mL$ .

Explanation:

Here, there is certainly 1:1 stoichiometry between acid and base, i.e.:

$N a O H (a q) + H C l (a q) \to N a C l (a q) + H_{2} O (l)$ $NaOH(aq) + HCl(aq) rarr NaCl(aq) + H_2O(l)$

And please note that the product $C_{1} V_{1} = moles \cdot L^{- 1} \times L$ $C_1V_1="moles"*L^-1xxL$ , i.e. an ANSWER in moles as required...........

And so if $C_{1} V_{1} = C_{2} V_{2}$ $C_1V_1=C_2V_2$ , then............

$V_{2} = \frac{C_{1} V_{1}}{C_{2}} = \frac{60 \cdot m L \times 0.15 \cdot m o l \cdot L^{- 1}}{0.500 \cdot m o l \cdot L^{- 1}} = 18 \cdot m L$ $V_2=(C_1V_1)/C_2=(60*mLxx0.15*mol*L^-1)/(0.500*mol*L^-1)=18*mL$

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A $60 \cdot m L$ $60mL$ volume of sodium hydroxide at $0.15 \cdot m o l \cdot L^{- 1}$ $0.15molL^-1$ concentration is titrated with $0.500 \cdot m o l \cdot L^{- 1}$ $0.500mol*L^-1$ $H C l (a q)$ $HCl(aq)$ . What volume of acid is required?

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Explanation:

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A 60⋅mL60*mL volume of sodium hydroxide at 0.15⋅mol⋅L−10.15*mol*L^-1 concentration is titrated with 0.500⋅mol⋅L−10.500*mol*L^-1 HCl(aq)HCl(aq). What volume of acid is required?

1 Answer

Explanation:

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A $60 \cdot m L$ $60mL$ volume of sodium hydroxide at $0.15 \cdot m o l \cdot L^{- 1}$ $0.15molL^-1$ concentration is titrated with $0.500 \cdot m o l \cdot L^{- 1}$ $0.500mol*L^-1$ $H C l (a q)$ $HCl(aq)$ . What volume of acid is required?