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yawa3891 [41]
3 years ago
14

What is the molar concentration (molarity) of 1.0 mol of KCl dissolved in 750 mL of

Chemistry
1 answer:
Nikolay [14]3 years ago
8 0

Answer:

Molarity is moles per liter. You have one mole in 0.750 liters

Explanation:

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Write the following measurement out of scientific notation. 2.345 x 10^-4 cm.
maw [93]
.0002345 I believe this is correct
7 0
3 years ago
The ksp of copper(ii) carbonate, cuco3, is 1.4 × 10-10. calculate the molar solubility of this compound.
mafiozo [28]
As,
                              CuCO₃    ⇆  Cu²⁺  +  CO₃²⁻
So,
                             Kc  =  [Cu²⁺] [CO₃²⁻] / CuCO₃
Or,
                             Kc (CuCO₃)  =  [Cu²⁺] [CO₃²⁻]
Or,
                             Ksp  =  [Cu²⁺] [CO₃²⁻]
As,
Ksp  = 1.4 × 10⁻¹⁰
So,
                            1.4 × 10⁻¹⁰  =  [x] [x]
Or,
                             x²  =  1.4 × 10⁻¹⁰ 
Or,
                             x  =  1.18 × 10⁻⁵ mol/L
To cahnge ito g/L,
                             x  =  1.18 × 10⁻⁵ mol/L × 123.526 g/mol

                   
         x  =  1.45 × 10⁻³ g/L
3 0
3 years ago
Change 0.00765 kL into mL
bagirrra123 [75]

Answer:

7650

Explanation:

formula- multiply the volume value by 1e+6

4 0
3 years ago
Read 2 more answers
If 17.8 grams of KOH dissolve in enough water to make a 198-gram solution, what is the concentration in percent by mass?
sleet_krkn [62]
Solute of solution = 17.8 g

Solvn = 198 g

% = 17.8 / 198

w% = 0.089 x 100 = 8.9%  by mass

hope this helps!
7 0
3 years ago
A solution prepared by mixing 10 ml of 1 m hcl and 10 ml of 1.2 m naoh has a ph of
blagie [28]

Answer: pH of resulting solution will be 13

Explanation:

pH is the measure of acidity or alkalinity of a solution.

Moles of H^+ ion = Molarity\times {\text {Volume in L}}=1M\times 0.01L=0.01mol

Moles of OH^- ion = Molarity\times {\text {Volume in L}}=1.2M\times 0.01L=0.012mol

HCl+NaOH\rightarrow NaCl+H_2O

For neutralization:

1 mole of H^+ ion will react with 1 mole of OH^- ion

0.01 mol of H^+  ion will react with =\frac{1}{1}\times 0.01mole of OH^- ion

Thus (0.012-0.01)= 0.002 moles of OH^- are left in 20 ml or 0.02 L of solution.

[OH^-]=\frac{0.002}{0.02L}=0.1M

pOH=-log[OH^-]

pOH=-log[0.1]=1

pH+pOH=14

pH=14-1=13

Thus the pH of resulting solution will be 13

7 0
3 years ago
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