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12.85
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What is the pOH of a solution with OH-1.4 10-13?
12.85 is the pOH.
What is the pOH of a solution with OH 1.4 10-13?
12.85
What is the pOH of a solution with OH- 1.4 x 10-13?
12.85
What is the pOH of a solution with [OH-] = 1.4 x 10-13?
12.85
What is the pOH of a solution with OH 1.4 10 13?
The pOH of a solution with an OH- concentration of 1.4 x 10^-13 M is 1.85. This is calculated by taking the negative logarithm of the OH- concentration, which is -log(1.4 x 10^-13) = 12.85, then subtracting it from 14 to find the pOH: 14 - 12.85 = 1.85.
What is the pH of 0.067 0 M KOH solution?
The pH of a 0.0670 M KOH solution can be calculated using the formula pH = 14 - pOH. Since KOH dissociates completely in water to produce OH- ions, the pOH can be found by taking the negative logarithm of the hydroxide ion concentration (0.0670 M in this case). Then, pH = 14 - pOH, allowing you to determine the solution's pH.
A solution has a pOH of 4.5 What is the hydroxide ion concentration of this solution?
The hydroxide ion concentration can be calculated using the formula: ( [\text{OH}^-] = 10^{-\text{pOH}} ). Plugging in 4.5 for pOH, we get ( [\text{OH}^-] = 10^{-4.5} = 3.16 \times 10^{-5} , \text{M} ).
How is the pH and poh of 0.1 M HCl?
For a 0.1 M HCl solution, all of the HCl molecules will dissociate into H+ and Cl- ions, resulting in a concentration of 0.1 M for H+ ions. Since pH = -log[H+], the pH of the solution is 1. The pOH can be calculated by subtracting the pH from 14, so the pOH would be 13.
How do you calculate OH- with a ph of 1.12?
To calculate the concentration of hydroxide ions (OH-) from a given pH value, you can use the formula: [OH-] = 10^(-pH). For a pH of 1.12, the concentration of hydroxide ions would be [OH-] = 10^(-1.12) = 0.079 moles per liter.
When was Alef Poh-ji born?
Alef Poh-ji was born on 1987-04-13.
What is molarity poh and pH of 4.50G of NaOH if diluted in up to 750 ml of H2O?
MW NaOH is 23+16+1 = 40. 4.5g in 750ml is 6.0g in 1L. Molarity is 6/40 = 0.15 OH- concentration is 0.15, pOH is -log100.15 = 0.82 H+ concentration is 10-14/0.15 = 6.67x10-13 pH is -log10 6.67x10-13 = 12.18
How would OH- in an ammonia solution compare with OH- in a sodium hydroxide solution of a similar concentration?
Molar concentration in both base solutions NH3 and NaOH is assumed to be (equal) 0.1 mol Base/LWeak base like ammonia (NH3) with pKb = 9.2 and concentration (assumed) Cb = 0.1 (mol/L)pOH = 0.5*[pKb + pCb] = 0.5*[9.2 + 1.0] = 5.1 , hence [OH-] = 7.9*10-6pH = 14 - pOH = 8.9 hence [H+]= 1.3*10-9Strong base hydroxide (like from NaOH) with concentration (equally assumed) Cb = 0.1 (mol/L)pOH = 1.0 because [OH-] = 0.1pH = 13.0 hence [H+]= 1.0*10-13
