what is the pH of coffee if the [H3O+] is 1*10^-5 M?

pH = -log(H3O^+)

Substitute and solve for pH.

Well, when it comes to coffee, it's like a balancing act. The pH of coffee can vary depending on factors like the type of coffee beans, brewing method, and the water used. But if we're talking about a general ballpark, with a [H3O+] concentration of 1*10^-5 M, you might find coffee somewhere in the slightly acidic range. So, let's just say coffee can definitely be "brew-tifully" acidic!

To determine the pH of coffee, we can use the formula:

pH = -log[H3O+]

Given that [H3O+] is 1x10^-5 M, we can substitute this value into the formula:

pH = -log(1x10^-5)

We can simplify this further:

pH = -log(1) - log(10^-5)

Since the logarithm of 1 is 0, the equation becomes:

pH = 0 - (-5)

Therefore, the pH of coffee with [H3O+] concentration of 1x10^-5 M is 5.

To determine the pH of coffee based on the concentration of H3O+ ions, we can use the formula:

pH = -log[H3O+]

Given that the [H3O+] is 1 * 10^-5 M, we can substitute this value into the formula:

pH = -log(1 * 10^-5)

Now let's solve it step by step:

1. The logarithm of a number in scientific notation can be split into two parts: the coefficient and the exponent. In this case, it is -5. So the equation becomes:

pH = -(log(1) + log(10^-5))

2. The logarithm of 1 is equal to 0, so the equation becomes:

pH = -(0 + log(10^-5))

3. The logarithm of 10^-5 can be simplified to -5, so the equation becomes:

pH = -(-5)

4. Negating a negative number gives us a positive number, so the equation becomes:

pH = 5

Therefore, the pH of coffee, given a [H3O+] of 1 * 10^-5 M, is 5.