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Which expression represents the concentration of OH- in sloution?
The concentration of hydroxide ions (OH⁻) in a solution can be represented as [OH⁻]. This concentration can be determined using the formula: [OH⁻] = Kw / [H⁺], where Kw is the ion product of water (1.0 x 10⁻¹⁴ at 25°C) and [H⁺] is the concentration of hydrogen ions in the solution. Alternatively, in basic solutions, [OH⁻] can be calculated directly from the pOH using the relation [OH⁻] = 10^(-pOH).
Which of these solutions are acidic a solution with OH equals 2.5 10-9 H plus equals 1.2 10 -4 H plus equals 3.4 10-8 pH equals 4.5 OH equals 1.0 10-4?
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
What is the pH of a solution with a H plus equals 10 -8?
2
What is the pH of a solution with H plus equals 2.3 10-12?
- log(2.3 X 10 -12 ) = 11.6 pH -----------------very little H + concentration in this solution.
What is the pH of a solution with an H plus equals 1.2 x 10-5?
-log(1.2 X 10^-5 M H(+)) = 4.9 pH H(+)
A solution has H plus equals 4.1 x 10-9 What is the pOH of this solution?
5.6
What is the H plus in a solution with pOH of 0.253?
To find the [H+] concentration in a solution with a pOH of 0.253, you first need to find the pOH of the solution which is 14 - pOH = 14 - 0.253 = 13.747. Then, you can use the relation [H+][OH-] = 1.0 x 10^-14 to calculate the [H+] concentration. [H+] = 10^-13.747 = 1.93 x 10^-14 M.
The sum of pH plus pOH?
The sum of pH and pOH is always equal to 14 in a neutral solution at 25°C. This is because pH is a measure of the concentration of H+ ions in a solution while pOH is a measure of the concentration of OH- ions. In a neutral solution, the concentration of H+ ions is equal to the concentration of OH- ions, resulting in a sum of 14.
A solution has H 3.2 10 7 What is the pOH of this solution?
7.5
A solution has H plus equals 6.2 x 10-3 What is the pOH of this solution?
7.8
A solution of HCl has H 2.5 x 10-5 What is the pOH of this solution?
pH + pOH = 14 If the pH is 3.4, the pOH is 10.6
What is the solution's pH and pOH?
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
When the H in a solution is 1.7 109 M what is the pOH?
To find the pOH of a solution when the H concentration is 1.7 x 10^-9 M, you can first calculate the pH using the formula: pH = -log[H+]. Then, you can find the pOH by subtracting the pH from 14, since pH + pOH = 14 in water. So, if the H concentration is 1.7 x 10^-9 M, the pH is 8.77, and the pOH is 14 - 8.77 = 5.23.
What is the pH and pOH of a 0.0067M HON3 solution?
Since HNO3 is a strong acid, it completely dissociates in solution. HNO3 -> H+ + NO3-. Therefore, the concentration of H+ ions is the same as the concentration of the HNO3 solution, 0.0067M. pH = -log[H+] = -log(0.0067) ≈ 2.18. pOH = 14 - pH ≈ 11.82.
If a solution had a pOH equals 10.7 what would be the H plus?
If an aqueous solution has a pOH value of 10.7 and is at standard temperature and pressure, the pH value is 14 - 10.7 = 3.3. From the definition of pH, this means that the logarithm (to base 10) of the molar concentration of H+, [H+] is -3.3. This can be written as +0.7 - 4. The antilog of 0.7 is 5, to the justified number of significant digits. Therefore, [H+] = 5 X 10-4.
Does the pH of a neutral solution at room temperature equal the pOH of the solution?
yes. because the ph of a neutrasl solution is 7. Meaning, the pOH of the solution is 7 7=7
What is the poH of 0.2 moles of sulphuric acid?
First u need to know the pH of sulfuric acid: ph= -log[h+] =-log[0.4] 0.3979 now u can find out the POH of sulfuric acid ph+poh=14 poh=14-0.3979 poh=13.6
