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Neko [114]
3 years ago
13

Please enter the values you calculated for each of your three trials for the molarity of your NaOH solution. Place your molarity

entries in the order corresponding with the masses of KHP and the volumes of NaOH required for the trials. You should enter 4 significant figures, e.g. 0.1487 M .
Entry # grams KHP mL NaOH M NaOH
#1: 0.5240 15.7 ?
#2: 0.5320 17.8 ?
#3: 0.5120 16.7
Chemistry
1 answer:
Alexandra [31]3 years ago
6 0

Answer:

#1. M NaOH = 0.1634 M

#2. M NaOH = 0.1464 M

#3. M NaOH = 0.1501 M

Explanation:

  • molarity [=] mol/L

balanced reaction:

  • NaOH + KHP → KNaP + H2O

∴ molar mass KHP = 204.22 g/mol

#1:

∴ mass KHP = 0.5240 g

∴ volume NaOH = 15.7 mL = 0.0157 L

⇒ moles NaOH = (0.5240 g KHP)(mol/204.22 g KHP)(mol NaOH/mol KHP)

⇒ moles NaOH = 2.566 E-3 mol

⇒ M NaOH = (2.566 E-3 mol)/(0.0157 L) = 0.1634 M

#2:

∴ mass KHP = 0.5320 g

∴ volume NaOH = 17.8 mL = 0.0178 L

⇒ moles NaOH = 2.605 E-3 mol

⇒ M NaOH = 0.1464 M

#3:

∴ mass KHP = 0.5120 g

∴ volume NaOH = 16.7 mL = 0.0167 L

⇒ moles NaOH = 2.5071 E-3 mol

⇒ M NaOH = 0.1501 M

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4 0
3 years ago
A solution was prepared by dissolving 0.800 g of sulfur S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and
sammy [17]

<u>Answer:</u> The freezing point of solution is 16.5°C and the boiling point of solution is 118.2°C

<u>Explanation:</u>

To calculate the molality of solution, we use the equation:

Molality=\frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ in grams}}

Where,

m_{solute} = Given mass of solute (S_8) = 0.800 g

M_{solute} = Molar mass of solute (S-8) = 256.52 g/mol

W_{solvent} = Mass of solvent (acetic acid) = 100.0 g

Putting values in above equation, we get:

\text{Molality of solution}=\frac{0.800\times 1000}{256.52\times 100.0}\\\\\text{Molality of solution}=0.0312m

  • <u>Calculation for freezing point of solution:</u>

Depression in freezing point is defined as the difference in the freezing point of water and freezing point of solution.

\Delta T_f=\text{freezing point of acetic acid}-\text{Freezing point of solution}

To calculate the depression in freezing point, we use the equation:

\Delta T_f=iK_fm

or,

\text{Freezing point of acetic acid}-\text{Freezing point of solution}=iK_fm

where,

Freezing point of acetic acid = 16.6°C

i = Vant hoff factor = 1 (for non-electrolyte)

K_f = molal freezing point depression constant = 3.59°C/m

m = molality of solution = 0.0312 m

Putting values in above equation, we get:

16.6^oC-\text{freezing point of solution}=1\times 3.59^oC/m\times 0.0312m\\\\\text{Freezing point of solution}=16.5^oC

Hence, the freezing point of solution is 16.5°C

  • <u>Calculation for boiling point of solution:</u>

Elevation in boiling point is defined as the difference in the boiling point of solution and freezing point of pure solution.

The equation used to calculate elevation in boiling point follows:

\Delta T_b=\text{Boiling point of solution}-\text{Boiling point of acetic acid}

To calculate the elevation in boiling point, we use the equation:

\Delta T_b=iK_bm

or,

\text{Boiling point of solution}-\text{Boiling point of acetic acid}=iK_fm

where,

Boiling point of acetic acid = 118.1°C

i = Vant hoff factor = 1 (for non-electrolyte)

K_f = molal boiling point elevation constant = 3.08°C/m

m = molality of solution = 0.0312 m

Putting values in above equation, we get:

\text{Boiling point of solution}-118.1^oC=1\times 3.08^oC/m\times 0.0312m\\\\\text{Boiling point of solution}=118.2^oC

Hence, the boiling point of solution is 118.2°C

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Percent error is the difference between the measured and known value, divided by the known value, multiplied by 100%.

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Finally, multiply your answer by 100

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Round to three significant figures, and you're done.

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