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Alex73 [517]
3 years ago
12

A solution containing 75.0 mL of 0.150 M strong acid (HCl) is titrated with 75.0 mL of 0.300 M strong base (NaOH). What is the p

H of the resulting solution
Chemistry
1 answer:
Alborosie3 years ago
7 0

Answer:

12.875

Explanation:

Balanced equation of the reaction:

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

mole of acid = mole of base

75 × 0.150 = volume of base needed × 0.3

volume of base needed = 37.5 ml

excess OH = 0.3 × 37.5 ml / 150 ml where total volume = 75 ml + 75 ml = 150 ml

excess OH = 0.075 M

pOH = - log (OH⁻) = - log (0.075 M) = 1.125

pH + pOH = 14

pH = 14 - pOH = 14 - 1.125 = 12.875

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bonufazy [111]
Thank you for posting your math problem here. To convert 3.9x10^5mg to dg the answer is <span>3.9 x 10^3 dg. Below is the solution: 

Solution:

</span><span>1mg=0.01dg 
</span><span> dg= 3.9 X 10^5mg
</span>dg = <span>(3.9 X 10^5) x 0.01
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7 0
3 years ago
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A chemist needs 0.550 mol selenium for a reaction. What mass of selenium should a chemist use?
-BARSIC- [3]

Answer:

The chemist would require to use 43.43 grams.

Explanation:

In order to solve this problem we need to know<u> how much do 0.550 moles of selenium weigh</u>. To do that we use selenium's<em> molar mass </em>and multiply it by the given number of moles:

  • 0.550 mol * 78.96 g/mol = 43.43 g

The chemist would require to use 43.43 grams.

4 0
3 years ago
How many moles of nitroge are there in 50.0 g of nitrogen?
chubhunter [2.5K]

1.785714286 moles

The number of moles (n) for nitrogen is: [ n=50.0÷28.0 ] = 1.785714286 moles.

8 0
3 years ago
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g) + 2H2(g) ⇌ C2H6(
sukhopar [10]

Answer:

-255.4 kJ

Explanation:

The free energy of a reversible reaction can be calculated by:

ΔG = (ΔG° + RTlnQ)*n

Where R is the gas constant (8.314x10⁻³ kJ/mol.K), T is the temperature in K, n is the number of moles of the products (n =1), and Q is the reaction quotient, which is calculated based on the multiplication of partial pressures by the partial pressure of the products elevated by their coefficient divide by the multiplication of the partial pressure of the reactants elevated by their coefficients.

C₂H₂(g) + 2H₂(g) ⇄ C₂H₆(g)

Q = pC₂H₆/[pC₂H₂ * (pH₂)²]

Q = 0.261/[8.58*(3.06)²]

Q = 3.2487x10⁻³

ΔG = -241.2 + 8.314x10⁻³x298*ln(3.2487x10⁻³)

ΔG = -255.4 kJ

4 0
3 years ago
Determine the heat energy needed to raise the temperature of 120 grams of ice at -5 to steam at 115°
CaHeK987 [17]

Answer:

Q = 30355.2 J

Explanation:

Given data:

Mass of ice = 120 g

Initial temperature = -5°C

Final temperature = 115°C

Energy required = ?

Solution:

Specific heat capacity of ice is = 2.108 j/g.°C

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

Q = m.c. ΔT

ΔT = T2 -T1

ΔT = 115 - (-5°C)

ΔT = 120 °C

Q = 120 g × 2.108 j/g.°C × 120 °C

Q = 30355.2 J

5 0
3 years ago
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