Strong Acids and Bases Calculator

pH and pOH Formulas:

\[ \text{pH} = -\log[\text{H}^+] \quad \text{or} \quad \text{pOH} = -\log[\text{OH}^-] \]

pH: Acidity (dimensionless)
pOH: Basicity (dimensionless)
[H⁺]: Hydrogen ion concentration (mol/L)
[OH⁻]: Hydroxide ion concentration (mol/L)

pH:

pOH:

[H⁺]:

[OH⁻]:

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1. What is a Strong Acids and Bases Calculator?

Definition: This calculator determines pH, pOH, and ion concentrations for strong acids and bases.

Purpose: It helps chemistry students and professionals quickly calculate solution properties without manual logarithmic calculations.

2. How Does the Calculator Work?

The calculator uses the formulas:

\[ \text{pH} = -\log[\text{H}^+] \quad \text{and} \quad \text{pOH} = 14 - \text{pH} \] \[ \text{pOH} = -\log[\text{OH}^-] \quad \text{and} \quad \text{pH} = 14 - \text{pOH} \]

For Strong Acids:

pH = -log[H⁺] where [H⁺] equals the acid concentration
pOH = 14 - pH
[OH⁻] = 10^-pOH

For Strong Bases:

pOH = -log[OH⁻] where [OH⁻] equals the base concentration
pH = 14 - pOH
[H⁺] = 10^-pH

3. Importance of pH Calculation

Details: pH measurements are critical in chemical reactions, biological systems, water treatment, and many industrial processes.

4. Using the Calculator

Tips: Enter the concentration in mol/L and select whether it's a strong acid or base. The calculator will provide all related values.

5. Frequently Asked Questions (FAQ)

Q1: What's considered a strong acid or base?
A: Strong acids (like HCl, H₂SO₄) and bases (like NaOH, KOH) completely dissociate in water.

Q2: Why is the pH scale logarithmic?
A: The logarithmic scale allows representation of the wide range of H⁺ concentrations (10⁻¹ to 10⁻¹⁴ mol/L) in a manageable 0-14 scale.

Q3: What's the relationship between pH and pOH?
A: pH + pOH = 14 at 25°C due to the water autoionization constant (Kw = 1×10⁻¹⁴).

Q4: Can I use this for weak acids/bases?
A: No, weak acids/bases don't completely dissociate, requiring different calculations involving Ka/Kb.

Q5: What's a neutral pH?
A: pH 7 (equal H⁺ and OH⁻ concentrations of 1×10⁻⁷ mol/L each) at 25°C.