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## How do you find the pH of the Nernst equation?

The formula for ph is pH = -log[H+}, so you can find the concentration of hydrogen ions by the Nearst equation.

## What is the relation between pH and potential?

So, we have the following conditions: As the pH decreases, the solution is more acidic, so 10−pH=[H+] increases and 10pH−14=[OH−] decreases. If H+ is a product, Q therefore increases, and the nonstandard cell potential decreases. If H+ is a reactant, Q therefore decreases, and the nonstandard cell potential increases.

Does cell potential depend on pH?

In those reactions in which H+ or OH– ions take part, the cell potential will also depend on the pH. Plots of E vs. pH showing the stability regions of related species are very useful means of summarizing the redox chemistry of an element.

Does pH affect Nernst equation?

pH doesn’t affect the Nernst equation. But the Nernst equation predicts the cell potential of reactions that depend on pH. If H⁺ is involved in the cell reaction, then the value of E will depend on the pH.

### What is the pH formula?

To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression: pH = – log [H3O+].

### Does pH affect Nernst Equation?

What does Nernst Equation tell you?

The Nernst Equation enables the determination of cell potential under non-standard conditions. It relates the measured cell potential to the reaction quotient and allows the accurate determination of equilibrium constants (including solubility constants).

What is the importance of Nernst equation?

The Nernst Equation allows for cell potential determination under non – standard conditions. It relates the measured cell potential to the quotient of the reaction and allows the exact determination of constants of equilibrium (including constants of solubility).

## How do you solve Nernst equation?

The Nernst Equation allows us to calculate the voltage produced by any electrochemical cell given E o values for its electrodes and the concentrations of reactants and products. The general Nernst Equation: E = E o -(RT/nF)lnQ. E o = standard electrochemical cell potential (voltage)

## What is the derivation for the Nernst equation?

The Nernst Equation is derived from the Gibbs free energy under standard conditions. (1) E o = E r e d u c t i o n o − E o x i d a t i o n o Δ G is also related to E under general conditions (standard or not) via (2) Δ G = − n F E

How does temperature affect the Nernst equation?

Temperature doesn’t affect the Nernst equation. Temperature is part of the Nernst equation: #E_”cell” = E_”cell”^° – (RT)/(zF)lnQ#. It shows that #E_”cell”# decreases as #T# increases if #Q# ≠ 1 and everything else stays constant.

How to calculate cell potential?

Calculating Standard Cell Potentials List the known values and plan the problem. Known E0 Ag = + 0.80V E0 Sn = − 0.14V Unknown E0 cell =? Solve. oxidation (anode): Sn(s) → Sn2 + (aq) + 2e − reduction(cathode): Ag + (aq) + e − → Ag(s) Before adding the two reactions together, the number Think about your result.