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

A scientist spilled a few drops of dilute hydrochloric acid (hcl) on a lab table. for safety purposes, the scientist sprinkled s

leonid [27]

Hello!

The observation that would provide the best evidence that a chemical reaction occurred is that The baking soda and hydrochloric acid combined, and bubbles formed.

When baking soda (NaHCO₃) and Hydrochloric Acid (HCl) combine, the following reaction happens:

NaHCO₃ + HCl → NaCl + H₂O + CO₂(g)↑

The gaseous Carbon Dioxide (CO₂) generated in this reaction is the responsible for the bubbles. The releasing of this gas is an evidence that a chemical reaction occurred between NaHCO₃ and HCl.

Have a nice day!

3 0

3 years ago

Write a balanced equation for the decomposition reaction described, using the smallest possible integer coefficients. When ammon

MAXImum [283]

Answer:

NH₄Cl ------> NH₃ + HCl

Explanation:

Ammonium Chloride =(NH₄Cl

Ammonia = NH₃

Hydrochloric Acid = HCl

NH₄Cl ------> NH₃ + HCl

In decomposition reaction, the reactant is breaking down into smaller parts. In this case, all of the coefficients are 1. The reaction is already balanced.

7 0

1 year ago

What is the volume of stank of nitrogen that contains 17 moles of nitrogen at 34 C under 12,000Pa?

Otrada [13]

Answer:

3626.76dm³

Explanation:

Given parameters:

Number of moles of Nitrogen in tank = 17moles

Temperature of the gas = 34°C

Pressure on the gas = 12000Pa

Unkown:

Volume of the tank, V =?

Converting the parameters to workable units:

We take the temperature from °C to Kelvin

K = 273 + °C = 273 + 34 = 307k

Taking the pressure in Pa to atm:

101325Pa = 1atm

12000Pa = 0.118atm

Solution:

To solve this problem, we employ the use of the ideal gas equation. The ideal gas law combines three gas laws which are the Boyle's law, Charles's law and the Avogadro's law.

It is expressed as PV = nRT

The unknown is the Volume and we make it the subject of the formula

V = $\frac{nRT}{P}$

Where R is called the gas constant and it is given as 0.082atmdm³mol⁻¹K⁻¹

Therefore V = $\frac{17 x 0.082 x 307 }{0.118}$ = 3626.76dm³

3 0

3 years ago

Read 2 more answers

The effectiveness of nitrogen fertilizers depends on both their ability to deliver nitrogen to plants and the amount of nitrogen

densk [106]

Answer:

Ammonia > Urea > Ammonium nitrate > Ammonium sulphate

Explanation:

Percentage by mass of nitrogen in NH3:

Molar mass of NH3= 17 g/mol

Hence % by mass = 14/17 × 100 = 82.35%

% by mass of NH4NO3

Molar mass of NH4NO3 = 80.043 g/mol

Hence; 28/80.043 × 100 = 34.98%

% by mass of (NH4)2SO4;

Molar mass of (NH4)2SO4= 132.14 g/mol

Hence; 28/132.14 × 100 = 21.19%

% by mass of CH4N2O

Molar mass of urea = 60.0553 g/mol

Hence 28/60.0553 × 100 = 46.62%

8 0

3 years ago

When 35.0 mL of 0.400 M hydrobromic acid and 35.0 mL of 0.400 M ammonia are combined, the pH of the resulting solution will be :

Kay [80]

Answer:

B. Equal to 7.

Explanation:

Hydrobromic acid is a strong acid that decreases pH and ammonia is a strong base that increases pH.

As the initial pH of water is 7,0 the addition of 35.0mL of 0.400M HBr will produce a pH less than 7,0. But, the same effect of decreasing pH is reverted for the addition of 35.0mL of 0.400M HNO3.

That means the net effect of the two addition is to have a pH:

B. Equal to 7.

I hope it helps!

3 0

3 years ago