I need a calculation for the hydrogen concentration (in mol litre-1) when 0.32g of nitric acid is dissolved in sufficient water to make 0.050 litres of final solution. Can I have the answer in scientific notation to an appropiate number of sig figures. I need to give reasoning for the above.
I also need the pH for this solution to the nearest whole number.
2007-06-12 07:28:04 · 3 answers · asked by R T 1 in Science & Mathematics ➔ Mathematics
MW HNO3 = 1 + 14 + 16*3 = 63
(0.32 grams)/(63 grams/mole) = 0.0051 moles HNO3
(0.0051 moles)/(0.050 liters) = 0.10 moles/liter
HNO3 -> H(+) + NO3(-)
pH = -log[H+]
pH = -log[0.1] = 1.0
HNO3 is a strong acid and will disassociate completely, so 0.1 moles of acid will yield 0.1 moles of hydrogen ions and a solution with a 0.1 molar hydrogen ion concentartion has a pH of exactly 1.
2007-06-12 07:40:27 · answer #1 · answered by Roger S 7 · 0⤊ 0⤋
0.32/1.51 = 0.021 lit nitric acid
0.32/63 = 5.1E-3 mol nitric acid
0.050 - 0.021 = 0.029 lit H2O
0.029 * 1000/18 = 1.6 mol H20
The solution contains 5.1E-3 + 2*1.6 = 3.2 mol H
The contribution of H by HNO3 is negligible
The solution contains 3.2/0.05 = 64 mol/lit of H
2007-06-12 07:41:36 · answer #2 · answered by gebobs 6 · 0⤊ 0⤋
It will make CO2 gas.
2016-04-01 03:50:24 · answer #3 · answered by Anonymous · 0⤊ 0⤋