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vaieri [72.5K]
3 years ago
8

a quantity of 18.68 mL of KOH solution is needed to neutralize 0.4218 g of KHP. What is the concentration (in molarity) of the K

OH solution?
Chemistry
1 answer:
SashulF [63]3 years ago
5 0
To neutralize an acidic substance with the basic solution, the number of moles should be equal. First, we calculate for the number of moles of KHP.

molar mass of KHP = (1 mol K)(39.1 g K/1 mol K) + (1 mol H)(1 g H/1 mol H) + (1 mol P)(30.97 g P / 1 mol P) = 71.07 g KHP/ mol

number of moles KHP = (0.4218 g KHP) x (1 mol KHP / 71.07 g KHP)
        n = 0.0059 moles

Let M be the molarity of the solution and equating the number of moles,
     0.0059 moles = (18.68 mL)(1 L/1000 mL)(M)
            M = 0.32 moles/L

<em>ANSWER: 0.32 M</em>
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2 years ago
Which one of the following statements is not true concerning 2.00 L of a 0.100 M solution of Ca3(PO4)2?
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<u>Answer:</u> The correct answer is Option B.

<u>Explanation:</u>

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

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}     .......(1)

  • <u>For A:</u>

Molarity of calcium phosphate solution = 0.100 M

Volume of solution = 2.00 L

Putting values in equation 1, we get:

0.100M=\frac{\text{Moles of }Ca_3(PO_4)_2}{2.00}\\\\\text{Moles of }Ca_3(PO_4)_2=(0.100mol/L\times 2.00L)=0.200mol

Moles of calcium phosphate = 0.200 moles

  • <u>For B:</u>

1 mole of calcium phosphate contains 3 moles of calcium atoms, 2 moles of phosphate atoms and 8 moles of oxygen atoms.

So, 0.200 moles of calcium phosphate will contain = (8\times 0.200)=1.6 moles of oxygen atoms.

Moles of oxygen atoms = 1.6 moles

  • <u>For C:</u>

Molarity of calcium phosphate solution = 0.100 M

Volume of solution = 1.00 L

Putting values in equation 1, we get:

0.100M=\frac{\text{Moles of }Ca_3(PO_4)_2}{1.00}\\\\\text{Moles of }Ca_3(PO_4)_2=(0.100mol/L\times 1.00L)=0.100mol

Moles of calcium ions = (0.100\times 3)=0.300 moles

  • <u>For D:</u>

Molarity of calcium phosphate solution = 0.100 M

Volume of solution = 5.00 L

Putting values in equation 1, we get:

0.100M=\frac{\text{Moles of }Ca_3(PO_4)_2}{5.00}\\\\\text{Moles of }Ca_3(PO_4)_2=(0.100mol/L\times 5.00L)=0.500mol

Moles of phosphorus atoms = (0.500\times 2)=1.00 moles

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1 mole of a compound contains 6.022\times 10^{23} number of atoms

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  • <u>For E:</u>

1 mole of calcium phosphate contains 3 moles of calcium ions and 2 moles of phosphate ions.

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Moles of calcium ions = 0.600 moles

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