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What is the molar concentration of hydroxide ions in a solution with a pH of 6?
Find the concentration of H ions first..
[H+]= antilog -ph
Then, find [OH-]
[OH-]= 1*10^-14/[H+]
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To find the molar concentration of hydroxide ions ([OH-]) in a solution with a pH of 6, we first need to find the concentration of hydrogen ions ([H+]).
The concentration of hydrogen ions can be calculated using the formula: [H+] = antilog(-pH). The antilog function is the inverse of the logarithm function, so it can be obtained by raising 10 to the power of the negative pH value.
In this case, since the pH is 6, the calculation would be:
[H+] = antilog(-6)
Next, we can use the formula [OH-] = 1*10^-14 / [H+] to find the concentration of hydroxide ions. This formula is based on the fact that water dissociates into equal concentrations of hydrogen ions and hydroxide ions, and at 25°C, the product of their concentrations is always equal to 1*10^-14.
By substituting the value of [H+] we calculated into the formula, we can find [OH-].
I hope this explanation helps! Please let me know if you have any further questions.