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Why NaOH show pH 6 as it is base?
If this is the outcome of a (too) simplified calculation formula for pH of hydroxide solutions, then here is the 'missing' part to correct this 'false' answer (or outcome):pH = 14.0 - pOH = 14.0 - [-log(OH-)] (this is generally valid at room temperature 25oC)simplified: pH = 14.0 - [-log(OH-)] = 14.0 + log(NaOH) = 14-[log(10-8)]= 6almost (but sufficiently) correct: .... = 14.0 + log[(NaOH) + (1.0*10-7)] so by adding the amount of OH- ions, already present in pure water. This can NOT longer be ignored when NaOH concentration is very diluted, below 10-6 mol/L.So when pHoutcome < 8 for dilute bases it should be 'recalculated' by addition of 10-7 before taking any log !(The same is analogously valid for dilute acids when pHoutcome > 6)pHoutcome = 6 for this NaOH concentration (which appears to have been (NaOH) = 1.0*10-8) is lower than 8 so is to be corrected as follows:pH = 14.0 + log[(NaOH) + (1.0*10-7)] = 14 + log[1.0*10-8 + 1.0*10-7] == 14 + log[1.1*10-7] = 14 - 6.96 = 7.04 = 7.0(and not 6 as in the simplified formula outcome)
A solution with a pH of 8 has how many times fewer hydrogen ions than a solution with a pH of 6?
pH 8: [H+] = 10^-8 M pH 6: [H+] = 10^-6 M 10^-6 / 10^-8 = 10^2 = 100 Answer is 100 times fewer
How many times more acid is a solution with a pH of 4 than a solution of pH of 6?
pH 8: [H+] = 10^-8 M pH 6: [H+] = 10^-6 M 10^-6 / 10^-8 = 10^2 = 100 Answer is 100 times fewer
What is the pH of a solution with H 2.3 10 6?
5.64
What is the pH of a solution with H 2.310-6?
The pH of a solution is given by the formula pH = -log[H+]. Therefore, if the concentration of H+ ions is 2.3 x 10^-6 M, the pH of the solution would be 5.64.
A solution of NaOH has OH- 1.9 x 10-6 What is the pOH of this solution?
5.7
Why NaOH show pH 6 as it is base?
If this is the outcome of a (too) simplified calculation formula for pH of hydroxide solutions, then here is the 'missing' part to correct this 'false' answer (or outcome):pH = 14.0 - pOH = 14.0 - [-log(OH-)] (this is generally valid at room temperature 25oC)simplified: pH = 14.0 - [-log(OH-)] = 14.0 + log(NaOH) = 14-[log(10-8)]= 6almost (but sufficiently) correct: .... = 14.0 + log[(NaOH) + (1.0*10-7)] so by adding the amount of OH- ions, already present in pure water. This can NOT longer be ignored when NaOH concentration is very diluted, below 10-6 mol/L.So when pHoutcome < 8 for dilute bases it should be 'recalculated' by addition of 10-7 before taking any log !(The same is analogously valid for dilute acids when pHoutcome > 6)pHoutcome = 6 for this NaOH concentration (which appears to have been (NaOH) = 1.0*10-8) is lower than 8 so is to be corrected as follows:pH = 14.0 + log[(NaOH) + (1.0*10-7)] = 14 + log[1.0*10-8 + 1.0*10-7] == 14 + log[1.1*10-7] = 14 - 6.96 = 7.04 = 7.0(and not 6 as in the simplified formula outcome)
A solution with a pH of 8 has how many times fewer hydrogen ions than a solution with a pH of 6?
pH 8: [H+] = 10^-8 M pH 6: [H+] = 10^-6 M 10^-6 / 10^-8 = 10^2 = 100 Answer is 100 times fewer
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.
How many times more acid is a solution with a pH of 4 than a solution of pH of 6?
pH 8: [H+] = 10^-8 M pH 6: [H+] = 10^-6 M 10^-6 / 10^-8 = 10^2 = 100 Answer is 100 times fewer
What is the pH of a solution with H 2.3 10 6?
5.64
What is the pH of a solution with H 2.310-6?
The pH of a solution is given by the formula pH = -log[H+]. Therefore, if the concentration of H+ ions is 2.3 x 10^-6 M, the pH of the solution would be 5.64.
A solution of HBr has H plus equals 2.1 x 10-6 What is the pH of this solution?
1.70
What is solution of pH 4 is 10 times more acidic than one of pH 5 and it is 10 times more acidic than a solution of pH 6 how many times more acidic is the solution of pH for than the one of pH 6?
No, a pH of 5 is ten times more acidic than a pH o6.
How much more acidic is a solution with a pH of 2 than one with a pH of 6 How much more basic is a solution with a pH of W than one with a pH of W?
From pH=2 to pH=6 the factor 1is 10 000. The factor is 10 for one unit of pH.
A solution with a pH of 7 is how many times more alkaline than one with a pH of 6?
100 times more Hydrogen ions are in solution of pH=5 as compare to pH=7.
What is the PH of a solution with and H plus of 3.7x10-6?
The pH of a solution can be calculated using the formula pH = -log[H+]. Substituting the given H+ concentration (3.7x10-6) into the formula gives pH = -log(3.7x10-6) ≈ 5.43. Therefore, the pH of the solution is approximately 5.43.
