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notka56 [123]
3 years ago
12

Suppose 2.57g of nickel(II) chloride is dissolved in 350.mL of a 38.0mM aqueous solution of potassium carbonate.

Chemistry
1 answer:
zepelin [54]3 years ago
4 0

Answer:

Molarity Ni^2+ = 0.0566 M

Explanation:

Step 1: Data given

Mass of nickel(II) chloride = 2.57 grams

volume of an aqueous 38.0 mM solution of potassium carbonate = 350 mL =0.350 L

The molar mass of nickel (II) chloride = 129.6 g/mol

Step 2: The balanced equation

NiCl2(aq) + K2CO3(aq) → 2KCl(aq) + NiCO3(s)

The dissociation of nickel (II) chloride:

NiCl2 →  Ni^2+ + 2Cl-

Step 3: Calculate moles NiCl2

Moles NiCl2 = mass NiCl2 / molar mass NiCl2

Moles NiCl2 = 2.57 grams / 129.6 g/mol

Moles NiCl2 = 0.0198 moles

For 1 mol NiCl2 we have 1 mol Ni^2+

For 0.0198 moles NiCl2 we have 0.0198 moles Nickel(II) cation

Step 4: Calculate molarity Ni^2+

Molarity Ni^2+ = moles / volume

Molarity Ni^2+ = 0.0198 moles / 0.350 L

Molarity Ni^2+ = 0.0566 M

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balu736 [363]

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Explanation:

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3 years ago
A sample of gas has a volume of 20.0 mL at STP. What will the volume be if the temperature is changed to 546 K and the pressure
Ostrovityanka [42]

The volume did not change, it remained at 20 ml

<h3>Further explanation</h3>

Given

20 ml a sample gas at STP(273 K, 1 atm)

T₂=546 K

P₂=2 atm

Required

The volume

Solution

Combined gas Law :

\tt \dfrac{P_1.V_1}{T_1}=\dfrac{P_2.V_2}{T_2}

Input the value :

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5 0
3 years ago
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