Calculate the approximate volume of 10 % (w/w) aqueous sodium carbonate that wil

Question

Calculate the approximate volume of 10 % (w/w) aqueous sodium carbonate that will be needed to neutralize the total amount of sulfuric acid i.e 1.5 ml..

a. What is the safety precaution to pay attention to during this step?

b. Write the complete balanced equation for the reaction between the two (acid and base)?

c. Calculate how many moles of the carbonate needed to just neutralize the acid. Show your work?

d. Calculate how many grams of the carbonate needed to just neutralize the acid. Show your work?

e. Approximate the volume of 10 % (w/w) aqueous sodium carbonate that will be required to neutralize the total amount of sulfuric acid. Show your calculations?

I am willing to post these questions speratley as long as someone will consistently answer them. Thank You!

Explanation / Answer

a.safety

Neutralisation should be performed at zero deg C. Mixing should be done slowly.

b. H2SO4 + 2NaHCO3 = Na2SO4 + 2CO2 + 2H2O

c. Moles of sodium bicarbonate needed

From the balanced equation we can see that one mole of H2SO4 requires two moles of sodium bicarbonate.

Mass of H2SO4 = VOLEME × DENSITY

= 1.5 ml × 1.84 g/ml = 2.76 g

Purity of H2SO4 = 98%

ACTUAL MASS OF H2SO4 = 0.98 × 2.76 = 2.70 g

Number of moles of H2SO4 = 2.70/98 = 0.0276 mol

Number of moles of sodium bicarbonate = 2× 0.0276

= 0.0552 mol

d. Amount of sodium bicarbonate = moles × molar mass

= 0.0552 × 84.007

= 4.64 g

e. Volme of solution required

10 g of sodium bicarbonate is present in 100 g of solution

Amonut of water = 100 -10 = 90 g

Volme of water = 90 ml

Since, 10 g sodium bicarbonate is present 90 ml of solution

4.64 g will be in : 90 × 4.64/10 = 41.76 ml

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.