How do I calculate the amount of H+ ions contained in 1.5litres of pH 6 solution?

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How do I calculate the amount of H+ ions contained in 1.5litres of pH 6 solution?

2006-12-05 02:03:18 · 3 answers · asked by Hannah B 1 in Science & Mathematics ➔ Chemistry

3 answers

pH = negative log of [H+]
pH = 6, so -log [H+] = 10^ -6 or .000001 moles/L

in 1.5 L there would be .0000015 moles [H+].

molecular weight of [H+] = 1 therefore 1g/mole or .0000015g [H+]

2006-12-05 02:17:13 · answer #1 · answered by davidosterberg1 6 · 0⤊ 0⤋

H+ ions concentration is 10^-pH
so 10^-6 mol of H+ ions per L
so in 1.5L, 1.5*10^-6 mol

2006-12-05 10:09:47 · answer #2 · answered by Anonymous · 0⤊ 0⤋

By definition, pH = - log [concentration H+ ions]

Therefore,

6 = - log [H+ ions]
[H+ ions] = 10^-6 moles / liter

Since we have 1.5 litres, then:

10^-6 moles / liter * 1.5 liters = 1.5 * 10^-6 moles (or 0.0000015 moles) H+ ions

2006-12-05 10:14:36 · answer #3 · answered by sep_n 3 · 0⤊ 0⤋