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2 years ago

What is the density of an object with 525 grams and a volume of 15cm3?

Chemistry

2 answers:

Hunter-Best [27]2 years ago

7 0

Answer: 35 g/cm

Explanation:

Density equals mass over volume. 525 divided by 15 is 35

victus00 [196]2 years ago

6 0

Answer:

35 g/cm

Explanation:

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Calculate the ph of a solution formed by mixing 200.0 ml of 0.30 m hclo with 300.0 ml of 0.20 m kclo. the ka for hclo is 2.9 × 1

masha68 [24]

Answer:

The pH of the solution will be 7.53.

Explanation:

Dissociation constant of KClO= $K_a=2.8\times 10^{-8}$

Concentration of acid in 1 l= 0.30 M

Then in 200 ml = $0.30 M\times 0.200 L=0.06 M$

The concentration of acid, HClO=[acid]= 0.006 M

Concentration of salt in 1 L = 0.20 M

Then in 300 ml = $0.20 M\times 0.300 L=0.06 M$

The concentration of acid, KClO=[salt]= 0.006 M

The pH of the solution will be given by formula :

$pH=pK_{a}^o+\log\frac{[salt]}{[acid]}$

$pH=-\log[2.8\times 10^{-8}]+\frac{[0.06 M]}{[0.06 M]}$

The pH of the solution will be 7.53.

4 0

3 years ago

Read 2 more answers

The density of an aqueous solution of nitric acid is 1.64 g/mL and the concentration is 1.85 M. What is the concentration of thi

galina1969 [7]

Answer:

Mass % of the solution = 7.1067 %

Explanation:

Given :

Molarity of nitric acid solution = 1.85 M

Density of the solution = 1.64 g/mL

Molarity of a solution is defined as the number of moles of solute present in 1 liter of the solution.

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

Lets, consider the volume of the solution = 1 L

Thus,

Moles of nitric acid present in the solution:

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

$Moles of Nitric acid=Molarity \times {Volume\ of\ the\ solution}$

So,

Moles of Nitric acid = 1.85 moles

Molar mass of nitric acid = 63 g/mol

The mass of Nitric acid can be find out by using mole formula as:

$moles=\frac{Mass\ taken}{Molar\ mass}$

Thus,

$Mass\ of\ Nitric\ acid=Moles \times Molar mass}$

$Mass\ of\ Nitric\ acid=1.85 g \times 63 g/mol}$

Mass of Nitric acid = 116.55 g

Also,

$Density=\frac{Mass}{Volume}$

Given : Density = 1.64 g/mL

Also, 1 L = 10³ mL

Volume of the solution is 1000 mL

So, mass of the solution:

$Mass\ of\ the\ solution=Density \times {Volume\ of\ the\ solution}$

$Mass\ of\ the\ solution=1.64 g/mL \times {1000 mL}$

Mass of the solution = 1640 g

Mass % is defined as the mass of solute in 100 g of the solution. The formula for the calculation of mass % is shown below:

$Mass \% =\frac{Mass\ of\ the\ solute}{Mass\ of\ the\ solution} \times {100}$

So,

$Mass \%=\frac{116.55}{1640} \times {100}$

Mass % = 7.1067 %

6 0

2 years ago

Chlorofluorocarbons photodissociate to produce chlorine atoms, cl•, which have been implicated in decreasing the concentration o

GrogVix [38]

Answer:

The role that chlorine atoms have in increasing the depeltion rate ozone is that Cl acts as a catalyst.

Explanation:

From the two steps of the reaction:

O₃ + Cl· → ClO· + O₂
ClO· + O → Cl· + O₂

The overall reaction is: O₃ + O → 2O₂

It is clear that ClO· is an intermediate that has been produced within the first step and has been consumed in the second step.

Also, Cl· is considered as a catalyst in this reaction that it has been consumed in the first step and has been produced in the second step, which means that it does not get up in the reaction, that is the main characteristic of the catalyst.

The catalyst usually increases the rate of the reaction by lowering its energy of activation (The minimum energy that is required to initiate the reaction) by proceeding the reaction in an alternative pathway (changing the reaction mechanism).

Hence, the role affecting the reaction rate that chlorine atoms have in increasing the depletion rate of ozone that it acts as a catalyst and does not get used up in the reaction.

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2 years ago

Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) with K2SO4(aq). Solubility Rules are found here.

wel

In ionic equations, the chemicals are written as the ions which are dissolved in water.

AgNO₃(aq) reacts with K₂SO₄(aq) and produces Ag₂SO₄(s) and KNO₃(aq). The balanced complete ionic reaction is
2Ag⁺(aq) + NO₃⁻(aq) +2K⁺(aq) + SO₄²⁻(aq) → Ag₂SO₄(s) +2K⁺(aq) + NO₃⁻(aq)

K⁺(aq) and NO₃⁻(aq) present in both sides. Hence, we can cut off them to find net ionic equation. So, net ionic equation is
2Ag⁺(aq) + SO₄²⁻(aq) → Ag₂SO₄(s)

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