Question
Calculate the volume of $0.083 \mathrm{M} \mathrm{HNO}_{2}$ that must be dissolved to make $1.00 \mathrm{~L}$ of a solution with a $\mathrm{pH}$ of 4.75
Step 1
Therefore, we can calculate the concentration of $\mathrm{H}^{+}$ ions required to produce a solution with a pH of 4.75 as follows: \[ [\mathrm{H}^{+}] = 10^{-\mathrm{pH}} = 10^{-4.75} = 1.78 \times 10^{-5} \, \mathrm{M} \] Show more…
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