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Zina [86]
3 years ago
14

A 50.00 mL sample of groundwater is titrated with 0.0800 M EDTA . If 10.90 mL of EDTA is required to titrate the 50.00 mL sample

, what is the hardness of the groundwater in molarity and in parts per million of CaCO 3 by mass
Chemistry
1 answer:
vitfil [10]3 years ago
4 0

Answer:

0.01744 M is the hardness of the groundwater.

1,744 ppm is the hardness of the groundwater in parts per million of calcium carbonate by mass.

Explanation:

Ca(In)^{2+}(red)+EDTA\rightarrow Ca(EDTA)^{2+}+In(blue)

In = Indicator

Concentration of calcium ion in groud water = C_1=?

Volume of ground water = V_1=50.00 mL

Concentration of EDTA solution = C_2=0.0800 M

Volume of EDTA solution = V_2=10.90 mL

C_1V_1=C_2V_2

C_1=\frac{C_2V_2}{V_1}=\frac{0.0800 M\times 10.90 mL}{50.00 mL}=0.01744 M

CaCO_3(sq)\rightarrow Ca^{2+}(aq)+CO_3^{2-}(aq)

[CaCO_3]=[Ca^{2+}]

So. [CaCO_3]=0.01744 M

0.01744 M is the hardness of the groundwater.

0.01744 Moles of calcium carbonate are present in 1 Liter of solution.

Mass of 0.01744 moles of calcium carbonate =

0.01744 mol\times 100=1.744 g

1 g = 1000 g

1.744 g = 1.744 × 1000 mg = 1,744 mg

ppm=\frac{\text{Mass of solute) mg)}}{\text{Volume of solution}{L}}

The hardness of the groundwater in parts per million :

\frac{1,744 mg}{1 L}= 1,744

1,744 ppm is the hardness of the groundwater in parts per million of calcium carbonate by mass.

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How many milliliters of a 17% benzalkonium chloride stock solution would be needed to prepare a liter of a 1:200 solution of ben
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Here is the complete question.

Benzalkonium Chloride Solution ------------> 250ml

Make solution such that when 10ml is diluted to a total volume of 1 liter a 1:200 is produced.

Sig: Dilute 10ml to a liter and apply to affected area twice daily

How many milliliters of a 17% benzalkonium chloride stock solution would be needed to prepare a liter of a 1:200 solution of benzalkonium chloride?

(A) 1700 mL

(B) 29.4 mL

(C) 17 mL

(D) 294 mL

Answer:

(B) 29.4 mL

Explanation:

1 L  =   1000 mL

1:200 solution implies the \frac{weight}{volume} in 200 mL solution.

200 mL of solution = 1g of Benzalkonium chloride

1000 mL will be \frac{1000mL}{200mL}=\frac{1g}{xg}

200mL × 1g = 1000 mL × x(g)

x(g) = \frac{200mL*1g}{1000mL}

x(g) = 0.2 g

That is to say, 0.2 g of benzalkonium chloride in 1000mL of diluted solution of 1;200 is also the amount in 10mL of the stock solution to be prepared.

∴ \frac{10mL}{250mL}=\frac{0.2g}{y(g)}

y(g) = \frac{250mL*0.2g}{10mL}

y(g) = 5g of benzalkonium chloride.

Now, at 17% \frac{weight}{volume} concentrate contains 17g/100ml:

∴  the number of milliliters of a 17% benzalkonium chloride stock solution that is needed to prepare a liter of a 1:200 solution of benzalkonium chloride will be;

= \frac{17g}{5g} = \frac{100mL}{z(mL)}

z(mL) = \frac{100mL*5g}{17g}

z(mL) = 29.41176 mL

≅ 29.4 mL

Therefore, there are 29.4 mL of a 17% benzalkonium chloride stock solution that is required to prepare a liter of a 1:200 solution of benzalkonium chloride

4 0
3 years ago
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