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3 years ago

What is the pH of a solution containing a 1.00 x 10−4 M solution of HCl?

Chemistry

1 answer:

ohaa [14]3 years ago

7 0

HCl = H⁺ + Cl⁻

c(HCl)=1.00*10⁻⁴ mol/l

[H⁺]=c(HCl)=1.00*10⁻⁴ mol/l

pH=-lg[H⁺]

pH=-lg(1.00*10⁻⁴)=4

pH=4

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$2 HBr (g) + 1/2 O_2 (g) \longrightarrow Br_2 (g) + H_2O (g)$

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(the 1.25 is because of the oxygen excess)

$n_{H_2O}=\frac{ 1 mol H_2O}{1 mol Br_2} *n_{Br_2}$

There is only one degree of freedom in this sistem, you can either deffine the moles of HBr you have or the moles of Br2 you want to produce. The other variables are all linked by the equations above.

b) Base of calculation 100 mol of HBr:

$nn_{HBr}=100 mol HBr$