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A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
Kclark71
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
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What is the Ph of a 0.0030 M HBr solution in water?
pH = - log10[H+] so 2.52
A solution of HBr has H plus equals 2.1 x 10-6 What is the pH of this solution?
1.70
What is the pH of 0.10 M HBr?
pH=1
If a solution of pH 6 was made into a solution of pH 3 the concentration of hydrogen ions would need to be?
1000 times increased. 106-3 = 103 =1000 because the pH scale is logarithmic.
What is the pH of 0.1 M HBr?
-log(0.1 M) = 1 pH
What is the Ph of a 0.0030 M HBr solution in water?
pH = - log10[H+] so 2.52
How do you determine the pH of a solution of 1.5 m of HBr?
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
A solution of HBr has H plus equals 2.1 x 10-6 What is the pH of this solution?
1.70
What is the pH of 0.10 M HBr?
pH=1
If a solution of pH 6 was made into a solution of pH 3 the concentration of hydrogen ions would need to be?
1000 times increased. 106-3 = 103 =1000 because the pH scale is logarithmic.
What is the pH of 0.1 M HBr?
-log(0.1 M) = 1 pH
What is the pH of a weak acid solution that has an H of 2.1 106 M?
pH = -log[H] = - log [2.1*10exp(-6)] = 5.68
What is the pH of HBr in Bromine water?
It depends on the concentration but this would be pretty acidic - pH of 0 -1 .
A 20.0ml sample of 0.800 m Hbr solution is titrated with 0.800 m NaOH solution calculate the pH of the solution after these volumes of base are added 12.5 ml 18.7 ml 20.0 ml 29.5 ml and 34.2?
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.
How many times more hydroxide ions are there in a solution with a pH than in a solution with a pH of 3?
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.
How many more hydroxide ions are there in a solution with a pH of 9 than in a solution with a pH of 3?
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.
How many times more hydroxide ions are in a solution with a pH of 9 than in a solution with a pH of 3?
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.
