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Ray Of Light [21]
3 years ago
10

In a titration experiment 12.5 ml of 0.500 m h2so4 neutralized 50.0 ml of naoh. the concentration of the naoh solution is ____.

Chemistry
1 answer:
s344n2d4d5 [400]3 years ago
4 0

0.250 mol/L

<em>Step 1</em>. Write the chemical equation

H2SO4 + 2NaOH → Na2SO4 + 2H2O

<em>Step 2</em>. Calculate the moles of H2SO4

Moles of H2SO4 = 12.5 mL H2SO4 × (0.500 mmol H2SO4/1 mL H2SO4)

= 6.25 mmol H2SO4

<em>Step 3</em>. Calculate the moles of NaOH

Moles of NaOH = 6.25 mmol H2SO4 × (2 mmol NaOH/(1 mmol H2SO4)

= 12.5 mmol NaOH

<em>Step 4</em>. Calculate the concentration of the NaOH

[NaOH] = moles/litres = 12.5 mmol/50.0 mL = 0.250 mol/L

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Read 2 more answers
How much heat is absorbed by a 112.5 g sample of water when it is heated from 12.5 °C to 9°C? (Specific heat capacity of water i
Oduvanchick [21]

Answer:

–1647.45 J

Explanation:

From the question given above, the following data were obtained:

Mass (M) = 112.5 g

Initial temperature (T₁) = 12.5 °C

Final temperature (T₂) = 9°C

Specific heat capacity (C) = 4.184 J/g°C

Heat (Q) absorbed =?

Next, we shall determine the change in temperature. This can be obtained as follow:

Initial temperature (T₁) = 12.5 °C

Final temperature (T₂) = 9°C

Change in temperature (ΔT) =?

ΔT = T₂ – T₁

ΔT = 9 – 12.5

ΔT = –3.5 °C

Finally, we shall determine the heat absorbed. This can be obtained as follow:

Mass (M) = 112.5 g

Change in temperature (ΔT) = –3.5 °C

Specific heat capacity (C) = 4.184 J/g°C

Heat (Q) absorbed =?

Q = MCΔT

Q = 112.5 × 4.184 × –3.5

Q = –1647.45 J

5 0
3 years ago
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