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What is the pH of HBr in Bromine water?
HBr in water will dissociate to form hydronium ions (H3O+) and bromide ions (Br-). The presence of water will increase the acidity, resulting in a pH of less than 7 for this solution. The exact pH would depend on the concentration of the HBr solution.
Is an aqueous solution of HBr acidic basic or neutral?
Its Acidic... HydroBromic Acid is acidic, even if you dilute it with water.
What is the pH of 0.1 M HBr?
The pH of a 0.1 M solution of HBr (hydrobromic acid) is around 1. It is a strong acid that dissociates completely in water to produce H+ ions, resulting in a low pH.
What is the pH of 0.10 M HBr?
The pH of 0.10 M HBr is approximately 1.0. HBr is a strong acid that completely dissociates in water to produce H+ ions, leading to a low pH value.
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 HBr in Bromine water?
HBr in water will dissociate to form hydronium ions (H3O+) and bromide ions (Br-). The presence of water will increase the acidity, resulting in a pH of less than 7 for this solution. The exact pH would depend on the concentration of the HBr solution.
Is an aqueous solution of HBr acidic basic or neutral?
Its Acidic... HydroBromic Acid is acidic, even if you dilute it with water.
What is the pH of 0.1 M HBr?
The pH of a 0.1 M solution of HBr (hydrobromic acid) is around 1. It is a strong acid that dissociates completely in water to produce H+ ions, resulting in a low pH.
What is the pH of 0.10 M HBr?
The pH of 0.10 M HBr is approximately 1.0. HBr is a strong acid that completely dissociates in water to produce H+ ions, leading to a low pH value.
Chemical Reaction between bromine and water?
When bromine reacts with water, it forms hydrobromic acid (HBr) and hypobromous acid (HOBr). The overall reaction can be represented as: Br2 + H2O → HBr + HOBr. This reaction is reversible and depends on the pH and conditions of the solution.
A solution of HBr has H plus equals 2.1 x 10-6 What is the pH of this solution?
1.70
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
When KOH is added to water what does the pH of the water solution do?
Increase pH (water) = 7 pH (KOH solution) is about 8 - 10
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
What sentence correctly describes a solution with a pH lower than the pH of distilled water?
A solution with a pH lower than the pH of distilled water is acidic. The pH of distilled water is 7, so any solution with a pH below 7 is considered acidic.
How an acid in the water solution affect the pH of the solution?
The pH is under 7.
