When concentrated sulfuric acid (18.0 M) is added to sodium chloride, hydrogen c

Question

When concentrated sulfuric acid (18.0 M) is added to sodium chloride, hydrogen chloride gas is formed.

H2SO4(l) +  NaCl(s)  ?  NaHSO4(s)  +  HCl(g)

When 50.0 mL of concentrated sulfuric acid is added to 1.15 g of sodium chloride, what volume (in mL) of hydrogen chloride gas is obtained at 1.00 atm pressure and 25oC?

Answer had : 2034ml which is incorrect what is the correct answer?

When a sample of oxalic acid (H2C2O4), which is a diprotic acid, is titrated with 0.250 M potassium hydroxide solution, 24.44 mL of the potassium hydroxide solution are required to neutralize the acid.  How many grams of oxalic acid where present in the sample?

2 KOH(aq)  +  H2C2O4(s) ?  K2C2O4(aq)  +  2 H2O(l)

Your answer should have 3 significant figures.

Answer had : 0.5499 gm which is incorrect what is the correct answer?

A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no more precipitate formed.  The precipitate is collected, dried, and weighed.  If 1.54 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample?

Answer had : 0.26M which is incorrect what is the correct answer?

Explanation / Answer

You need to determine the limiting reagent, which in this case is NaCl(sodium chloride); H2SO4 is in excess. The reaction shows that that 1 mole of reactants are needed to produce 1 mole of products (i.e., moles of the limiting reagent is equal to moles of reactants). Solve for moles of limiting reagent:

1 mole of NaCl=58.44g

1.15g*(1 mole/58.44g)=0.01968 moles of NaCl

0.01968 moles of NaCl=moles of HCl

Use the gas law which is the following:

PV=nRT

Where

P=pressure=1.00 atm
T=temperature (K)= 273.15 + C

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