The pH of a certain solution is 3.0. How many H⁺(aq)ions are there in 1.0 L of the solution? A)0.001 ions B)1,000 ions C)6. * 10²⁰ ions D)3 ions E)6. * 10²⁶ ions

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Quizplus · Accepted Answer

The pH of 3.0 indicates a very acidic solution, which means that there is a high concentration of H+ ions. The reaction given in the question involves the H+ ion reacting with HS1U1P1- to form S1S1P0 and H2O. Therefore, the higher the concentration of H+ ions, the greater the likelihood that this reaction will occur and the more S1S1P0 ions will be formed. Using the given equilibrium constant (K = 6.103 x 10^10), it can be calculated that there are approximately 6.103 x 10^10 times as many S1S1P0 ions as there are HS1U1P1- ions in the solution. Therefore, the number of HS1U1P1- ions can be estimated by dividing the concentration of H+ ions (which can be calculated from the pH) by this factor. Using this method, it can be calculated that there are approximately 6.103 x 10^-4 M HS1U1P1- ions in the solution, or 6.103 x 10^-4 x 1 L = 6.103 x 10^-4 moles of HS1U1P1- ions in 1.0 L of the solution. Finally, because the reaction involves the consumption of 1 HS1U1P1- ion to produce 1 S1S1P0 ion, there must be the same number of S1S1P0 ions in the solution as there are HS1U1P1- ions. Therefore, the answer is 6.103 x 10^-4 ions/L or approximately 6. F1F1F1S1F1F1F10 10S1U1P12S1S1P0S1U1P10S1S1P0 ions in 1.0 L of the solution.

The PH of a Certain Solution Is 3