a 1.00 l volume of hcl reacted completely with 2.00 l of 1.50 m ca(oh)2 according to the balanced chemical…

a 1.00 l volume of hcl reacted completely with 2.00 l of 1.50 m ca(oh)2 according to the balanced chemical equation below. 2hcl + ca(oh)2 → cacl2 + 2h2o what was the molarity of the hcl solution? 0.375 m 1.50 m 3.00 m 6.00 m

a 1.00 l volume of hcl reacted completely with 2.00 l of 1.50 m ca(oh)2 according to the balanced chemical equation below. 2hcl + ca(oh)2 → cacl2 + 2h2o what was the molarity of the hcl solution? 0.375 m 1.50 m 3.00 m 6.00 m

Answer

Answer:

D. 6.00 M

Explanation:

Step1: Calculate moles of Ca(OH)₂

$n_{Ca(OH)_2}=M\times V = 1.50\ mol/L\times2.00\ L=3.00\ mol$

Step2: Determine mole - ratio from equation

From $2HCl + Ca(OH)2\rightarrow CaCl_2 + 2H_2O$, the mole - ratio of $HCl$ to $Ca(OH)2$ is $n{HCl}:n{Ca(OH)_2}=2:1$.

Step3: Calculate moles of HCl

$n_{HCl}=2\times n_{Ca(OH)_2}=2\times3.00\ mol = 6.00\ mol$

Step4: Calculate molarity of HCl

$M_{HCl}=\frac{n_{HCl}}{V_{HCl}}=\frac{6.00\ mol}{1.00\ L}=6.00\ M$