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Zanzabum
3 years ago
13

Watch the video that shows using the dilution method to make a solution of known concentration. Note that while the video shows

the use of a beaker, in the lab we typically use a volumetric flask to make the diluted solution. The stock solution of KMnO4 has a concentration of 2.6 × 10-4 M. The pipette has a volume of 10.0 mL. What is the amount of KMnO4 delivered to the solution, in moles
Chemistry
1 answer:
Nady [450]3 years ago
4 0

Answer:

2.6\times 10^{-6}\ moles

Explanation:

Considering:

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

Or,

Moles =Molarity \times {Volume\ of\ the\ solution}

Given :

For potassium permanganate :

Molarity = 2.6\times 10^{-4}\ M

Volume = 10.0 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 10.0×10⁻³ L

Thus, moles of potassium sulfate :

Moles=2.6\times 10^{-4} \times {10.0\times 10^{-3}}\ moles

Moles of potassium permanganate = 2.6\times 10^{-6}\ moles

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Suppose of nickel(II) chloride is dissolved in of a aqueous solution of potassium carbonate. Calculate the final molarity of chl
stich3 [128]

Answer: Molarity of chloride anion = 0.32 M

<em>Note: the question is missing some values. The full question is given below;</em>

<em>Suppose 7.26 g of nickel(II) chloride is dissolved in 350 mL of a 0.50 M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits.</em>

Explanation:

Molarity or molar concentration is the number of moles (mol) of component per volume (liters) concentration of solution in mol/L or M

The mass of nickel (II) chloride is 7.26 g.

The volume of potassium carbonate is 350 mL = 0.35 L

The molarity of potassium carbonate solution is 0.50 M

The reaction of nickel (II) chloride and potassium carbonate is given below.

NiCl₂(aq) + KCO₃(aq) --------> KCl(aq) +NiCO₃(s)

The dissociation of nickel (II) chloride is given below.

NiCl₂   -----> Ni²⁺ + 2Cl⁻

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

The moles of nickel (II) chloride can be calculated by the formula given below;

No of moles  = mass(g) / molar mass (g/mol)

No of moles = 7.26 / 129.6 = 0.056 moles

Therefore, molarity of NiCl₂ = 0.056 moles/ 0.35 L = 0.16 M

The molarity of 1 mole nickel (ii) chloride is 0.16 m and according to dissociation of nickel (II) chloride, 1 mole of nickel (II) chloride gives 2 moles of chloride anion.

Therefore, the molarity of chloride anion = 0.16 * 2 = 0.32 M

3 0
3 years ago
Name the acid and base needed to form the salt ammonium nitrate give the chemical reaction
velikii [3]

Answer:

here

Explanation:

(NH4NO3), a salt of ammonia and nitric acid, ....4 and 3 are sub script

A neutralization reaction is a chemical reaction where an acid and a base are combined with the intent of producing a neutral pH level.

4 0
2 years ago
Read 2 more answers
Why are these graphs misleading
ch4aika [34]
Although there isn’t a picture a graph can be misleading when it doesn’t start at zero, it doesn’t give accurate information, it skips too many numbers, the vertical scale is too big or too small. Hope this helps
7 0
3 years ago
Please tell me what the answer is please
xenn [34]

Answer:

2

Explanation:

7 0
2 years ago
Read 2 more answers
A chemist prepares a solution of calcium sulfate (CaSO_4) by measuring out 0.0101 g of calcium sulfate into a 350. mL volumetric
Citrus2011 [14]

Answer:

2.123x10⁻⁴ M (mol/L)

Explanation:

First, we are considering the molar mass for each element, a data we obtain from the periodic table:

Ca= 40

S= 32

O= 16

Then, for CaSO₄, the molecular mass is 136 g per mol

As we dissolve 0.00101 g of this salt, we are going to convert this mass in moles units:

1 mol CaSO₄=136 g → 0.0101 g=7.43x10⁻⁵ mol

We finally obtain the concentration for the 350 ml, having in mind that it should be in mol/L:

350ml=7.43x10⁻⁵ mol

1000ml (1L)=2.123x10⁻⁴ M , where M=mol/L

3 0
3 years ago
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