Buffer Solutions
Chemistry ⇒ Acids, Bases, and Salts
Buffer Solutions starts at 11 and continues till grade 12.
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A buffer solution contains 0.3 M NH₄OH and 0.2 M NH₄Cl. Calculate the pH if K_b for NH₄OH is 1.8 × 10⁻⁵.
A buffer solution contains 0.4 M formic acid (HCOOH, pKₐ = 3.75) and 0.2 M sodium formate. Calculate the pH.
A buffer solution is made by mixing 0.1 M HCOOH and 0.1 M HCOONa. What will happen to the pH if a small amount of HCl is added?
A buffer solution is made by mixing 0.5 M acetic acid and 0.5 M sodium acetate. What is the pH if pKₐ = 4.76?
A buffer solution is prepared by mixing 0.1 mol of NH₄Cl and 0.1 mol of NH₄OH in 1 L of water. What is the pH if K_b for NH₄OH is 1.8 × 10⁻⁵? (pK_b = 4.74)
A buffer solution is prepared by mixing 0.2 mol of NH₄Cl and 0.1 mol of NH₄OH in 1 L of water. What is the pH? (K_b for NH₄OH = 1.8 × 10⁻⁵)
A buffer solution is prepared by mixing 0.25 mol of acetic acid and 0.25 mol of sodium acetate in 0.5 L of solution. What is the pH? (pKₐ = 4.76)
Calculate the pH of a buffer solution containing 0.2 M acetic acid (pKₐ = 4.76) and 0.1 M sodium acetate.
Define a buffer solution and give one example.
Describe how you would prepare 1 L of a buffer solution with pH 4.76 using acetic acid and sodium acetate.
Describe the composition of a buffer solution that can maintain a pH close to 5.
Explain why a buffer solution has a limited capacity to resist pH change.
Explain why a mixture of HCl and NaCl does not act as a buffer.
Explain why the buffer capacity is higher when the concentrations of the acid and its salt are high.
Explain why the pH of a buffer does not change significantly upon dilution.
State the effect on the pH of an acidic buffer when a small amount of strong base is added.
What is meant by the term 'buffer range'?
What is the effect of adding a strong acid to a basic buffer solution?
What is the main function of a buffer in blood plasma?
