Table of Contents
What is the pH of a solution of 10 2 M HBr solution?
The pH of 2.55×10−2 M HBr solution is pH = 1.59.
How do you find the pH of a solution with H+?
pH is defined by the following equation, pH = −log [H+] , where [H+] denotes the molar hydrogen ion concentration. Notice that we are required to take the common (base 10) logarithm of the hydrogen ion concentration in order to calculate pH.
What is the pH of a 1.5 x 10-10 HBr solution?
5) More challenging: What is the pH of a 1.5 x 10-10 HBr solution? If you do the calculation to find –log (1.5 x 10-10), you get an answer of 9.8.
What is the H+ concentration of pH 2?
Proper Definition of pH
| Molar Concentration of HCl | pH defined as Concentration | Experimentally Determined pH |
|---|---|---|
| 0.0100 | 2 | 2.04 |
| 0.100 | 1 | 1.10 |
| 0.40 | 0.39 | 0.52 |
| 7.6 | -0.88 | -1.85 |
Is HBr an acid or base?
Although the Br − ions derive from a strong acid (HBr), the NH 4 + ion derives from a weak base (NH 3), so the solution will be acidic, and NH 4Br is an acidic salt….11.5 Strong and Weak Acids and Bases and their Salts.
| Acids | Bases |
|---|---|
| HCl | LiOH |
| HBr | NaOH |
| HI | KOH |
| HNO 3 | RbOH |
What is the pH of a solution that has a H +] 0.0045 m?
The solution with [H+] = 0.0045 M will have a pH of 2.35.
What is the H+ ion concentration in a 2.1 x10 4 m Ca OH 2 solution?
The H+ ion concentration in the solution is 2.4×10-11 M.
How do you calculate H+ concentration?
Key Concepts
- The hydrogen ion concentration in a solution, [H+], in mol L-1, can be calculated if the pH of the solution is known.
- pH is defined as the negative logarithm (to base 10) of the hydrogen ion concentration in mol L-1 pH = -log10[H+]
- [H+] in mol L-1 can be calculated using the equation (formula): [H+] = 10-pH