CHEMISTRY HIGH SCHOOL

What would be the molar concentration of a 0.85% solution of sodium hypochlorite? (assume the density of solution to be 1.0 g/ml.)?

Answers

Answer 1
Answer:

The molar concentration of the solution 0.114 M.

We can obtain the molar concentration from the weight percent of solution using the formula;

CM = 10 C%w/w d/MM

Where;

CM = molar concentration

C%w/w = percent concentration

d = density

MM = molar mass

Substituting values, we have;

CM = 10 × 0.85 × 1.0 /74.44

CM = 0.114 M

Learn more: brainly.com/question/1340582

Answer 2
Answer: 0.11 M
   I am assuming that the 0.85% is by weight. So let's start with determining the molar mass of sodium hypochlorite (NaClO).
 Atomic weight sodium = 22.989769
 Atomic weight chlorine = 35.453
 Atomic weight oxygen = 15.999

   Molar mass NaClO = 22.989769 + 35.453 + 15.999 = 74.442 g/mol

   Now 1 liter of the solution will contain 1000 g * 0.0085 = 8.5 g.
 Moles NaClO = 8.5 g / 74.442 g/mol = 0.114182854 mol

   And since molarity is defined as moles per liter, the result (rounded to 2 significant digits) is 0.11 M

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When does incomplete combustion occur? A.
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B.
insufficient supply of carbon dioxide

C.
sufficient supply of carbon dioxide

D.
insufficient supply of oxygen

Answers

Answer:

D. insufficient supply of oxygen

Explanation:

Combustion is an exothermic reaction which involves the burning of a compound in the presence of oxygen. Combustion is a very useful life process as it produces heat and light.

For a complete combustion reaction to occur, the compound must be burnt over excess oxygen. The product is usually carbondioxide and water with release of some particulate matter.

In incomplete combustion, there is deficiency of oxygen. Here, oxygen becomes the limiting agent and it drives the reaction to an end. Incomplete combustion is always accompanied with the production of poisonous carbon monoxide and Carbon. We see incomplete combustion when smoke forms or when burning is accompanied by production of soot.

What makes a combustive process complete or not is the availability of oxygen gas for the reaction.

COLLEGE

It is desired to produce 2.25 grams of dichloromethane (CH2Cl2) by the following reaction. If the percent yield of dichloromethane (CH2Cl2) is 65.5 %, how many grams of carbon tetrachloride would need to be reacted? ______grams carbon tetrachloride

methane (CH4)(g) + carbon tetrachloride(g) dichloromethane (CH2Cl2)(g)

Answers

Answer:- 3.12 g carbon tetrachloride are needed.

Solution:- The balanced equation is:

From given actual yield and percent yield we will calculate the theoretical yield that would be further used to calculate the grams of carbon tetrachloride.

percent yield formula is:

percent yield =

theoretical = 3.44 g

From balanced equation, there is 2:1 mol ratio between dichloethane and carbon tetrachloride.

Molar mass of dichloroethane is 84.93 gram per mol and molar mass of carbon tetrachloride is 153.82 gram per mol.

=

So, 3.12 grams of carbon tetrachloride are needed to be reacted.

MIDDLE SCHOOL

Step by step on how to find limiting reactant, with an example please!

Answers

In order to find a limiting reactant, you'll at least need the mass of both reactants, or even better, number of moles of it (but you can work this out with the mass).

1. Write a balanced equation for the reaction. Balancing the equation is especially important because the mole ratio (the numbers when balancing) can affect the answer.

2. Find the number of moles of each reactant. You can find this by dividing the mass in grams by the molar mass of substance (adding all atomic masses of all elements present).

3.  Find the actual number of moles needed in the reaction by considering the mole ratio from the equation. Which means, if the mole ratio of reactant A : reactant B is 1:1, you don't need to change anything, but, if its somewhat 2:1 or 2:3 etc, you have to multiply or divide the n.o.m.s to make the mole ratio balanced. (You can refer to example if this part is a bit confusing)

4.  Determine which reactant has the least number of moles. That one is the limiting reactant!

Example (Question took from 2013 IGCSE Chemistry Paper3);

"4.8g of calcium is added to 3.6 g of water. The following reaction occurs.

Ca + 2H2O → Ca(OH)2 + H2

Find the limiting reactant."

1. The balanced equation is already given, so you're good for this step!

2. Find the n.o.m.s for the 2 reactants.

no. of moles of Ca

= 4.8 / 40.1

= 0.1197 mol

no. of moles of H2O

= 3.6 / (1.0 x 2 + 16.0)

= 0.2 mol

3. Consider the equation again,

From equation, mole ratio of Ca:H2O = 1:2

So, no. of moles of moles of Ca = 0.1197 x 2

= 0.2394 mol

4. Since 0.2 mol is less than 0.2394mol, H2O is the limiting reactant.

HIGH SCHOOL

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2. Both the ice cubes and water gain heat and energy
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4. The Ice Cube loses heat energy and the water gains heat energy

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observe that you were given the amounts of each substance in moles

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anther


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style

Answers

Hello,

Here is your answer:

The proper answer to this question is option C "stigma".

Here is how:

The stigma is responsible for producing pollen in a plant.

Your answer is C.

If you need anymore help feel free to ask me!

Hope this helps!
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Answers

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