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zvonat [6]
3 years ago
12

calculate how many milliliters of 0.142 M NaOH are needed to completely neutralize 21.4 mL of 0.294 M H2C4H4O6.

Chemistry
1 answer:
Flura [38]3 years ago
3 0

Answer:

The answer to your question is 88.7 ml

Explanation:

Data

Volume = ?

Concentration of NaOH = 0.142 M

Volume of H₂C₄H₄O₆ = 21.4 ml

Concentration of H₂C₄H₄O₆ = 0.294 M

Balanced chemical reaction

               2 NaOH + H₂C₄H₄O₆  ⇒  Na₂C₄H₄O₆  +  2H₂O

1.- Calculate the moles of H₂C₄H₄O₆

Molarity = moles/volume

Solve for moles

moles = Molarity x volume

Substitution

moles = 0.294 x 21.4/1000

Result

moles = 0.0063

2.- Use proportions to calculate the moles of NaOH

              2 moles of NaOH ------------------ 1 moles of H₂C₄H₄O₆

               x                           ------------------ 0.0063 moles

               x = (0.0063 x 2) / 1

               x = 0.0126 moles of NaOH

3.- Calculate the volume  of NaOH

Molarity = moles / volume

Solve for volume

Volume = moles/Molarity

Substitution

Volume = 0.0126/0.142

Result

Volume = 0.088 L or 88.7 ml

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An 80L capacity steel cylinder contains H2 at a pressure of 110 atm and 30 ° C, after extracting a certain amount of gas, the pr
icang [17]

Answer:

2200 L

Explanation:

Ideal gas law:

PV = nRT,

where P is absolute pressure,

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R is universal gas constant,

and T is absolute temperature.

The initial number of moles is:

(110 atm) (80 L) = n (0.0821 L atm / K / mol) (30 + 273.15) K

n = 353.58 mol

After some gas is removed, the number of moles remaining is:

(80 atm) (80 L) = n (0.0821 L atm / K / mol) (30 + 273.15) K

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The amount of gas removed is therefore:

n = 353.58 mol − 257.15 mol

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