Calculate the mass of HCL that need to prepare $200 \mathrm{ml}$ of solution?
$$
[\mathrm{H}+]=7.9 \backslash \text { times } 10^{\wedge}-3
$$

Question

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Calculate the number of moles of $\mathrm{H}^+$**: Given the concentration of $\mathrm{H}^+$ ions is $7.9 imes 10^{-3}$ M, we can calculate the number of moles in $200 \mathrm{ml}$ of solution. ‖ ‖ 2 ⋮ **Convert volume to liters**: $200 \mathrm{ml}$ is equivalent to $0.2$ liters since $1000 \mathrm{ml} = 1 \mathrm{l}$. ‖ ‖ 3 ⋮ **Use the molarity equation**: Molarity ($M$) is defined as the number of moles of solute ($n$) per liter of solution ($V$), so $n = M imes V$. ‖ ‖ 4 ⋮ **Calculate the mass of $\mathrm{HCl}$**: The molar mass of $\mathrm{HCl}$ is approximately $36.46 \mathrm{g/mol}$. Using the number of moles calculated, we can find the mass by multiplying the number of moles by the molar mass of $\mathrm{HCl}$. ‖ ∻Answer∻ ⚹ The mass of $\mathrm{HCl}$ needed is approximately $0.579 \mathrm{g}$. ⚹ ∻Key Concept∻ ⚹ Molarity and molar mass are used to calculate the mass of a solute needed to prepare a solution. ⚹ ∻Explanation∻ ⚹ By knowing the molarity and volume of the solution, we can find the number of moles of $\mathrm{H}^+$, which is equivalent to the moles of $\mathrm{HCl}$ needed. Multiplying this by the molar mass of $\mathrm{HCl}$ gives the mass required. ⚹◊What is the molarity of the HCL solution being prepared?⍭ Generate me a similar question◊

Sia