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pH = - log10[H+] so 2.52
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∙ 13y ago
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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 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
A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
What is the pH of 0.1 M HBr?
-log(0.1 M) = 1 pH
What is the pH of HBr in Bromine water?
It depends on the concentration but this would be pretty acidic - pH of 0 -1 .
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
How does the presence of an acid in a water solution affect of the pH of the solution?
The presence of an acid lowers the pH of the solution in water.
A solution of HBr has H 2.1 x 10-6 What is the pH of this solution?
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
How an acid in the water solution affect the pH of the solution?
The pH is under 7.
When KOH is added to water what does the pH of the water solution do?
The pH of water increase.
What is the pH of 0.1 M HBr?
-log(0.1 M) = 1 pH
What has a pH level of 11?
A pH=11 is a pH of a basic solution; for example a solution of sodium hydroxide in water.
What is the pH value of water solution?
It depends what you mean by water solution. If it's a solution of something else in water, it depends on the solute. If you mean just water, it's pH 7.
When a solution is neutralized its pH is brought to?
7.0, or the pH of water.
