By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31
Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
HBr being a strong monoprotic acid : [M] = [H+] = 2.62*10-2 and pH = -log[H+] =-log(2.62*10-2) = 1.582
5.7
10.7
1.58
pH = - log10[H+] so 2.52
1.70
pH=1
1000 times increased. 106-3 = 103 =1000 because the pH scale is logarithmic.
-log(0.1 M) = 1 pH
pH = - log10[H+] so 2.52
pH=-log[H+] pH-log(1.2x10^-3) pH=2.92 since the the pH plus the pOH is always equal 14 14-2.92=11.08 so the pOH is 11.08
1.70
pH=1
1000 times increased. 106-3 = 103 =1000 because the pH scale is logarithmic.
-log(0.1 M) = 1 pH
pH = -log[H] = - log [2.1*10exp(-6)] = 5.68
It depends on the concentration but this would be pretty acidic - pH of 0 -1 .
Looks as if you will need to calculate the pH of the final solution. The formula you need will be [H+] = 1 x 10-6 M.
The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.
The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.
The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.