The pH of a solution is 6.5 What are the [H+] and [OH-] of the solution?
[H+] = 6.5
[OH-] = 14-6.5=7.5
Come on, Newt.
pH=-log(H+)
antilog(-pH)=[H+] =antilog(-6.5)=http://www.rapidtables.com/calc/math/anti-log-calculator.htm=3.16 10^-7
and pOH=14-pH=7.5
OH concentration=antilog(-7.5) using same calculator..=3.16e-8
Well, if the pH of the solution is 6.5, then the [H+] would be equivalent to 10 to the power of negative 6.5. And since water is neutral, the [H+] would be equal to the [OH-] concentration. So, based on my calculations, this solution is probably as close to neutral as my chances of becoming a professional acrobat – pretty balanced!
To determine the [H+] and [OH-] of a solution with a pH of 6.5, we need to first understand the relationship between pH and the concentration of hydrogen ions ([H+]).
The pH scale is a logarithmic scale used to indicate the acidity or basicity of a solution. It is based on the concentration of hydrogen ions present. The pH scale ranges from 0 to 14, where a pH of 7 is considered neutral, pH less than 7 indicates acidity, and pH greater than 7 indicates basicity.
The equation for calculating pH is:
pH = -log[H+]
To find the concentration of hydrogen ions ([H+]), we can rearrange the equation as follows:
[H+] = 10^(-pH)
Given that the pH of the solution is 6.5, we can calculate [H+] using the equation:
[H+] = 10^(-6.5)
Calculating this, we find:
[H+] = 3.16 x 10^(-7)
Now, to find the concentration of hydroxide ions ([OH-]), we can use the equation for calculating the concentration of hydroxide ions in water:
[H+] x [OH-] = 1 x 10^(-14)
Rearranging the equation to solve for [OH-]:
[OH-] = (1 x 10^(-14)) / [H+]
For our given [H+], we can substitute the value to calculate [OH-]:
[OH-] = (1 x 10^(-14)) / (3.16 x 10^(-7))
Calculating this, we find:
[OH-] ≈ 3.16 x 10^(-8)
Therefore, the [H+] of the solution is approximately 3.16 x 10^(-7) and the [OH-] is approximately 3.16 x 10^(-8).
To find the [H+] and [OH-] concentrations of a solution given its pH, we can use the relationship between pH and [H+]. The pH scale is a logarithmic scale that measures the acidity or basicity of a solution. It is defined as the negative logarithm (base 10) of the hydrogen ion concentration ([H+]) in moles per liter.
The equation to convert pH to [H+] is:
[H+] = 10^(-pH)
Given that the pH of the solution is 6.5, we can substitute this value into the equation:
[H+] = 10^(-6.5)
Calculating this value, we get:
[H+] ≈ 3.16 x 10^(-7) mol/L
By doing a simple calculation, we can find the concentration of [OH-] using the equation for the ion product of water:
[H+] x [OH-] = 1.0 x 10^(-14) mol^2/L^2
Therefore:
[OH-] = (1.0 x 10^(-14)) / [H+]
Substituting the calculated [H+] value, we get:
[OH-] ≈ (1.0 x 10^(-14)) / (3.16 x 10^(-7))
Performing this calculation, we find:
[OH-] ≈ 3.16 x 10^(-8) mol/L
So, the [H+] concentration of the solution is approximately 3.16 x 10^(-7) mol/L, and the [OH-] concentration is approximately 3.16 x 10^(-8) mol/L.