All categories

2 years ago

In the titration of 82.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many mL of LiOH are required to reach the equivalence point

Chemistry

1 answer:

Igoryamba2 years ago

8 0

Answer:

218.7 mL

Explanation:

The reaction that takes place is:

HCOOH + LiOH → LiCOOH + H₂O

First we calculate how many HCOOH moles reacted, using the given volume and concentration:

82.0 mL * 0.400 M = 32.8 mmol HCOOH

As 1 HCOOH mol reacts with 1 LiOH mol, 32.8 mmoles of LiOH are needed to react with 32.8 mmoles of HCOOH.

Finally we calculate how many mL of a 0.150 M solution would contain 32.8 mmoles:

32.8 mmol / 0.150 M = 218.7 mL

You might be interested in

Which body tissue or organ contains the most mitochondria?

love history [14]

Muscle tissue has has the most mitochandria

4 0

3 years ago

Suppose of copper(II) acetate is dissolved in of a aqueous solution of sodium chromate. Calculate the final molarity of acetate

uranmaximum [27]

Answer:

0.0714 M for the given variables

Explanation:

The question is missing some data, but one of the original questions regarding this problem provides the following data:

Mass of copper(II) acetate: $m_{(AcO)_2Cu} = 0.972 g$

Volume of the sodium chromate solution: $V_{Na_2CrO_4} = 150.0 mL$

Molarity of the sodium chromate solution: $c_{Na_2CrO_4} = 0.0400 M$

Now, when copper(II) acetate reacts with sodium chromate, an insoluble copper(II) chromate is formed:

$(CH_3COO)_2Cu (aq) + Na_2CrO_4 (aq)\rightarrow 2 CH_3COONa (aq) + CuCrO_4 (s)$

Find moles of each reactant. or copper(II) acetate, divide its mass by the molar mass:

$n_{(AcO)_2Cu} = \frac{0.972 g}{181.63 g/mol} = 0.0053515 mol$

Moles of the sodium chromate solution would be found by multiplying its volume by molarity:

$n_{Na_2CrO_4} = 0.0400 M\cdot 0.1500 L = 0.00600 mol$

Find the limiting reactant. Notice that stoichiometry of this reaction is 1 : 1, so we can compare moles directly. Moles of copper(II) acetate are lower than moles of sodium chromate, so copper(II) acetate is our limiting reactant.

Write the net ionic equation for this reaction:

$Cu^{2+} (aq) + CrO_4^{2-} (aq)\rightarrow CuCrO_4 (s)$

Notice that acetate is the ion spectator. This means it doesn't react, its moles throughout reaction stay the same. We started with:

$n_{(AcO)_2Cu} = 0.0053515 mol$

According to stoichiometry, 1 unit of copper(II) acetate has 2 units of acetate, so moles of acetate are equal to:

$n_{AcO^-} = 2\cdot 0.0053515 mol = 0.010703 mol$

The total volume of this solution doesn't change, so dividing moles of acetate by this volume will yield the molarity of acetate:

$c_{AcO^-} = \frac{0.010703 mol}{0.1500 L} = 0.0714 M$

8 0

3 years ago

What would be the formula of the precipitate that forms when pb(no3)2 (aq) and k2so4 (aq) are mixed?

maria [59]

The formula of the ppt. formed is PbSo4 , which is inslouble.

6 0

3 years ago

A reaction of 17.0 g of ammonia with 26.6 g of chlorine gas

Elena-2011 [213]

Answer: if doing it on ck-12 the answer is 40.1

Explanation:

4 0

2 years ago

How many molecules are there in 1024 grams of Na2SO4?

tino4ka555 [31]

Answer:

1.91 x 450 molecules

Explanation:

4 0

3 years ago