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Calculate the pH of \(0.001\) molar solution of \(HCl\).
\(HCl\) is a and is in its solutions according to the
process:
process:
\(HCl_{(aq)}→ H^+_{(aq)}+Cl^–{(aq)}\)
From this process, it is clear that one mole of \(HCl\) would give one mole of \(H^+\) ions.
Therefore, the, i.e., \(0.001\) molar or \(1.0\times10^{–3}\) \(mol\) \(litre^{–1}\).
Thus, \([H^+] = 1\times10^{–3}\) \(mol\) \(litre^{–1}\)
\(pH = –log_{10}[X]\)
Where, X is
\(= –log_{10}10^{–3}\)
Thus, \(pH=\)
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