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If that is the hydronium ion concentration, then
-log(H+) = pH
negative natural common log10 of the H+concentration.
If this is the hydroxide ion concentration, there's a couple ways of going about it.
You could find the pOH = -log(OH-) and subtract it from 14
Or you could solve for the hydronium ion conc. and then take the negative log of the result.
Just remember p of anything (pH, pOH, pKa, etc) is just the negative natural common log of whatever number.
What else can I help you with?
What would be the pH of a solution with a hydrogen ion concentration of 0.00001 M?
The pH of a solution with a hydrogen ion concentration of 0.00001 M would be 5. The formula to calculate pH is pH = -log[H+], so in this case, pH = -log(0.00001) = 5.
Calculate concentration of hydroxide ion with given pH?
Ist step, calculate pOH value by using formula pH + pOH = 14 2nd step, pOH = -log[OH], [OH] = - Antilog of pOH
Calculate the molarity of HCl of pH 5.7?
To calculate the molarity of a solution from its pH, use the formula: pH = -log[H+]. In this case, pH 5.7 corresponds to [H+] = 1 x 10^-5.7 M. Given that HCl is a strong acid and dissociates completely in water, the molarity of HCl is also 1 x 10^-5.7 M.
How do you calculate the pH of a 0.001 M NaOH solution?
To calculate the pH of a 0.001 M NaOH solution, you can use the formula pH = 14 - pOH. Since NaOH is a strong base that completely dissociates in water, the pOH can be directly calculated as -log(0.001) = 3. Thus, the pH of the solution would be 14 - 3 = 11.
What is the pH of an acetic acid solution when 30 ml 0.15 m naoh have been added to 50 ml 0.1 m hoac?
To calculate the pH of the solution after mixing, first find the moles of acetic acid (HOAc) and NaOH. Then, determine which reactant is limiting to find the excess OH-. Use the excess OH- to calculate the concentration of OH- in the final solution, and then use this to calculate the pH.
Calculate the pH of 0.2 M HNO2 solution ( Ka = 4.5 * 10 -5 )?
pH= -log = 1.59
What would be the pH of a solution with a hydrogen ion concentration of 0.00001 M?
The pH of a solution with a hydrogen ion concentration of 0.00001 M would be 5. The formula to calculate pH is pH = -log[H+], so in this case, pH = -log(0.00001) = 5.
Calculate concentration of hydroxide ion with given pH?
Ist step, calculate pOH value by using formula pH + pOH = 14 2nd step, pOH = -log[OH], [OH] = - Antilog of pOH
Calculate the molarity of HCl of pH 5.7?
To calculate the molarity of a solution from its pH, use the formula: pH = -log[H+]. In this case, pH 5.7 corresponds to [H+] = 1 x 10^-5.7 M. Given that HCl is a strong acid and dissociates completely in water, the molarity of HCl is also 1 x 10^-5.7 M.
How do you calculate the pH of a 0.001 M NaOH solution?
To calculate the pH of a 0.001 M NaOH solution, you can use the formula pH = 14 - pOH. Since NaOH is a strong base that completely dissociates in water, the pOH can be directly calculated as -log(0.001) = 3. Thus, the pH of the solution would be 14 - 3 = 11.
What is the formula to calculate pH slope?
The formula to calculate pH slope is ΔpH/Δlog[H+], where ΔpH is the change in pH and Δlog[H+] is the change in the log concentration of hydrogen ions. This formula is used to determine the sensitivity of a pH electrode.
What is the pH of an acetic acid solution when 30 ml 0.15 m naoh have been added to 50 ml 0.1 m hoac?
To calculate the pH of the solution after mixing, first find the moles of acetic acid (HOAc) and NaOH. Then, determine which reactant is limiting to find the excess OH-. Use the excess OH- to calculate the concentration of OH- in the final solution, and then use this to calculate the pH.
What is the pH of 0.1 M propanoic acid?
The pH of a 0.1 M propanoic acid solution can be calculated using the dissociation constant (Ka) of propanoic acid, which is 1.3 x 10^-5. First, calculate the concentration of propanoate ions by solving for x in the equilibrium expression for propanoic acid. Then, calculate the pH using the formula pH = -log[H+], where [H+] is the concentration of protons in the solution.
Calculate pH of 1.0 m acetic acid?
The pH of a 1.0 M acetic acid solution is approximately 2.88. Acetic acid is a weak acid so it partially ionizes in water, resulting in the release of hydronium ions which lower the pH of the solution.
A 20.0ml sample of 0.800 m Hbr solution is titrated with 0.800 m NaOH solution calculate the pH of the solution after these volumes of base are added 12.5 ml 18.7 ml 20.0 ml 29.5 ml and 34.2?
To calculate the pH after each volume of NaOH is added, you need to determine the moles of HBr initially, moles of NaOH added, and then use these values to calculate the final concentration of H3O+ ions in the solution. From there, you can calculate the pH using the equation pH = -log[H3O+]. Repeat these calculations for each volume of NaOH added to find the pH at 12.5 ml, 18.7 ml, 20.0 ml, 29.5 ml, and 34.2 ml.
What is the pH of a 0.0110 M solution of Ba OH2?
The pH of a 0.0110 M solution of Ba(OH)2 can be calculated by finding the hydroxide ion concentration, which is double the concentration of the Ba(OH)2 solution. Therefore, [OH-] = 2 * 0.0110 M = 0.0220 M. From this, you can calculate the pOH using the formula -log[OH-], and then convert pOH to pH using the relation pH + pOH = 14.
What is the pH level of 0.0005 M HF solution?
The pH of a 0.0005 M HF (hydrofluoric acid) solution can be calculated using the formula: pH = -log[H+]. First, determine the concentration of H+ ions produced by HF dissociation and then calculate the negative logarithm of that concentration to find the pH.
