Q: What is the pH of a solution of 1.0 x 10 -3 M H30?

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-log(9.40 X 10^-4) = 3 pH

3: The negative of the logarithm (base 10) of the concentration. The logarithm of 1 is 0 and the logarithm of 10-3 is -3; the logarithm of their product is the sum of their individual logarithms, -3 in this instance, and the negative of -3 is +3.

-Log(1.4x10-3)= 2.85 The Log to be used here is the decimal one, not the neperian one.

- log(2.0 X 10 -3 M) = 2.7 pH ======

If you mean 10+2y = 16 then the solution is y = 3

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2.64

The pH of a 1.6x10^-3 M HNO3 solution is approximately 2.8. This is calculated by taking the negative logarithm (base 10) of the concentration of the hydrogen ions in the solution.

Remembwer pH is = the negative logarithm to base ten, of the hydrogen ion concentration . So with a concentration of 0.001 M The hydrogen ion concentration is 0.001 = 10^(-3) ph = -log(10)[H^+] pH = -log(10)10^-3 pH = -(-3) log(10)10 ( Remember log(10)10 = 1 ) pH = -(-3)(1) = --3 = 3 pH = 3

The concentration of hydrogen ions in a solution with a pH of 3 is 1 x 10^-3 mol/L.

The pH of a solution can be calculated using the formula pH = -log[H+]. Since the concentration of H+ in this case is 2.3 x 10^-3, the pH would be -log(2.3 x 10^-3) = 2.64.

To find the pH of the resultant solution, you can use the formula: pH = -log[H+]. Calculate the [H+] concentration for each solution using the pH values (pH 3 = 1.0 x 10^-3 M and pH 8 = 1.0 x 10^-8 M) and add them together. Then, convert the total [H+] concentration back to pH using the formula mentioned earlier.

1/103 = 0.001 M ========( pH 3 ) 1/105 = 0.00001 M ============( pH 5 ) As you see, a pH of 3 has a 100 times concentration of 5 pH ( 10 * 10 devalued ) This is the scale; logarithmic.

The pH scale is logarithmic, so each unit corresponds to a 10-fold difference in hydrogen ion concentration. Therefore, a solution with a pH of 9 has 1,000,000 (10^6) times more hydroxide ions than a solution with a pH of 3.

As the pH decreases, the solution becomes 10 times more acidic for each point. A solution of pH 4 is 10 times more acidic than a solution of pH 5. A solution of pH 3 is 10 times more acidic than a solution of pH 4. 10 x 10 = 100 A solution of pH 3 is 100 times more acidic than a solution of pH 5.

The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.

The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.

The concentration of hydroxide ion is realted to pH by the pKw (10-14) At pH 9 the concentration of OH- is 10-5, at pH 3, 10-11. The ratio is 106 so there are a million times as many OH- in pH 9.