How you would make 100.0 ml of a 1.00 mol/L buffer solution with a pH of 10.80 to be made using only sodium carbonate, sodium hydrogen carbonate and water? How much sodium carbonate and sodium hydrogen carbonate would you use?
You would add 7.96 g of sodium carbonate and 2.09 g of sodium hydrogen carbonate to a volumetric flask and then add enough water to make the volume up to 100.0 mL.
This question is like the question in
https://tutor.hix.ai
1. Calculate the concentration ratios
The chemical equation for the equilibrium is
HCO₃⁻ + H₂O ⇌ CO₃²⁻ + H₃O⁺;
HA + H₂O ⇌ A⁻ + H₃O⁺
The Henderson-Hasselbalch equation is
pH = 10.80 = 10.32 + This makes sense. pH > 2. Calculate the concentrations [A⁻] = 3.02[HA] Also, [A⁻] + [HA] = 1.00 mol/L 3.02[HA] + [HA] = 4.02[HA] = 1.00 mol/L [HA] = [A⁻] = 3.02[HA] = 3.02 × 0.2488 mol/L = 0.7512 mol/L 3. Calculate the masses of NaHCO₃ and of Na₂CO₃ Mass of NaHCO₃ = 0.1000 L × Mass of Na₂CO₃ = 0.1000 L × You would transfer 2.09 g of NaHCO₃ and 7.96 g of Na₂CO₃ to a 100 mL volumetric flask and make up to the mark with distilled water.
By signing up, you agree to our Terms of Service and Privacy Policy
To make 100.0 ml of a 1.00 mol/L buffer solution with a pH of 10.80 using only sodium carbonate (Na2CO3), sodium hydrogen carbonate (NaHCO3), and water, you would mix the two components in such a way that the resulting solution has the desired pH. To calculate the amounts needed, you'd use the Henderson-Hasselbalch equation. First, determine the ratio of the concentrations of the conjugate base (Na2CO3) to the weak acid (H2CO3), which is the desired buffer system. Then, use this ratio to find the amounts of each compound needed to prepare the buffer solution.
By signing up, you agree to our Terms of Service and Privacy Policy
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- When #HCl# and #NH_3# are mixed why is the buffer #NH_3-NH_4Cl#?
- What is a buffer in chemistry?
- How many milliliters of 0.20N sodium hydroxide must be added to 75 mL of 0.050 N hydrochloric acid to make a neutral solution?
- How would #"barium nitride"# react with water?
- If 525 mL of 0.80 M HCl solution is neutralized with 315 mL of Sr(OH)2 solution what is the molarity of the Sr(OH)2? __ HCl + __ Sr(OH)2 __ SrCl2 + __ H2O

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7