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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

Answer :

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

The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change.

NaOH + KHP → KNaP + H2O

According to the question, the molar mass is KHP = 204.22 g/mol

  • mass KHP = 0.5240 g

volume NaOH = 15.7 mL = 0.0157 L

moles NaOH =[tex]0.5240*204.22[/tex]

moles NaOH = 2.566.

Molarity is NaOH =[tex]= \frac{2.566}{0.0157} =0.1634[/tex]

  • mass KHP = 0.5320 g

[tex]volume NaOH = 17.8 mL = 0.0178 Lmoles NaOH = 2.605 molM NaOH = 0.1464 M[/tex]

  •  mass KHP = 0.5120 g

[tex]volume NaOH = 16.7 mL = 0.0167 Lmoles NaOH = 2.5071 molM NaOH = 0.1501 M[/tex]

Hence, the molarity of the following is 0.1501M.

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https://brainly.com/question/20486415

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