All categories

3 years ago

If 32.3 grams of KCl are dissolved in 192 grams of water, what is the concentration of the solution in percent by mass?

Chemistry

2 answers:

vichka [17]3 years ago

6 0

Answer:

The concentration of the solution in percent by mass is 14.3%

Explanation:

Given:

Mass of KCl (solute) = 32.3 g

Mass of water (solvent) = 192 g

To determine:

Concentration of solution in % mass i,e. %(w/w)

Formula:

%w/w $= \frac{Mass\ of\ solute}{Total\ mass\ of\ solution } *100\\$

Total mass of solution = solute + solvent = 32.3 + 192 = 224.3 g

%w/w = $\frac{32}{224.3} *100 = 14.3%$

Likurg_2 [28]3 years ago

3 0

The concentration is 0.168 g/ml

You might be interested in

Can any one help on this one

enyata [817]

0.004382166 Make sure to round to the right amount of Sig Figs

8 0

3 years ago

A solution of KMnO4 has an absorbance of 0.539 when measured in the colorimeter. Determine the concentration of the KMnO4 given

loris [4]

Answer:

Concentration of unknown solution is 0.0416 M

Explanation:

As we know

Absorbance is equal to the product of molar absorptivity of KMnO4 m, path length and concentration

From the given set of graphical data, it is clear that the absorbance vs concentration is a straight line.

From the graph, we can obtain-

Y = 5.73 X – 0.0065

Absorbance = 0.232

0.232 = 5.73 X – 0.0065

X = 0.0416

Concentration of unknown solution is 0.0416 M

6 0

2 years ago

How many liters of carbon dioxide will be produced at STP if 3.56 g calcium carbonate reacts completely with carbon dioxide? CaC

sp2606 [1]

Answer:

V = 0.798 L

Explanation:

Hello there!

In this case, for this gas stoichiometry problem, we first need to compute the moles of carbon dioxide via stoichiometry and the molar mass of starting calcium carbonate:

$3.56gCaCO_3*\frac{1molCaCO_3}{100gCaCO_3} *\frac{1molCO_2}{1molCaCO_3} =0.0356molCO_2$

Next, we use the ideal gas equation for computing the volume, by bearing to mind that the STP conditions stand for a pressure of 1 atm and a temperature of 273.15 K:

$PV=nRT\\\\V=\frac{nRT}{P}\\\\V=\frac{0.0356mol*0.08206\frac{atm*L}{mol*K}*273.15K}{1atm} \\\\V=0.798L$

Best regards!

4 0

2 years ago

Which substances will make a salt when combined?

babymother [125]

The answer is D. Fertilizer and vinegar

3 0

3 years ago

Read 2 more answers

The melting point of H₂O(s) is 0 °C. Would you expect the melting point of H₂S(s) to be 85 °C, 0 °C or -85 °C.? Justify your cho

dimulka [17.4K]

Answer:

-85 °C

Explanation:

O and S are in the same group( Group 16). Since S is below O it's atomic mass is higher than O. So molar mass of H2S is higher than H2O. The strength of Vanderwaal Interactions ( London dispersion forces) increases when the molar mass increases. However, only H2O can form H bonds with each other. This is because electronegativity of O is higher than S and therefore H in H2O has a higher partial positive charge than H of H2S.

H bond dominate among these 2 types of forces so the strength of attractions between molecules is higher in H2O than H2S. Therefore more energy should be supplied for H2O to break inter

molecular forces and convert from solid to liquid state than H2S. So mpt of H2O must be higher than that of H2S.

5 0

2 years ago