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3 years ago

What is the difference between a heterogeneous mixture and homogeneous mixture?

Chemistry

1 answer:

Fiesta28 [93]3 years ago

7 0

A homogeneous mixture has the same uniform appearance and composition throughout

A heterogeneous mixture consists of visibly different substances or phases.

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What mass of potassium hypochlorite (FW-90.6 g/mol) must be added to 4.50 x 10 mL of water to give a solution with pH 10.20? [Ka

marta [7]

Answer : The mass of potassium hypochlorite is, 4.1 grams.

Explanation : Given,

pH = 10.20

Volume of water = $4.50\times 10^2ml=0.45L$

The decomposition of KClO will be :

$KClO\rightarrow K^++ClO^-$

Now the further reaction with water $(H_2O)$ to give,

$ClO^-+H_2O\rightarrow HClO+OH^-$

First we have to calculate the pOH.

$pH+pOH=14\\\\pOH=14-pH\\\\pOH=14-10.20=3.8$

Now we have to calculate the $OH^-$ concentration.

$pOH=-\log [OH^-]$

$3.8=-\log [OH^-]$

$[OH^-]=1.58\times 10^{-4}M$

Now we have to calculate the base dissociation constant.

Formula used : $K_b=\frac{K_w}{K_a}$

Now put all the given values in this formula, we get :

$K_b=\frac{1.0\times 10^{-14}}{4.0\times 10^{-8}}=2.5\times 10^{-7}$

Now we have to calculate the concentration of $ClO^-$ .

The equilibrium constant expression of the reaction is:

$K_b=\frac{[OH^-][HClO]}{[ClO^-]}$

As we know that, $[OH^-]=[HClO]=1.58\times 10^{-4}M$

$2.5\times 10^{-7}=\frac{(1.58\times 10^{-4})^2}{[ClO^-]}$

$[ClO^-]=0.0999M$

Now we have to calculate the moles of $ClO^-$ .

$\text{Moles of }ClO^-=\text{Molarity of }ClO^-\times \text{Volume of solution}$

$\text{Moles of }ClO^-=0.0999mole/L\times 0.45L=0.0449mole$

As we know that, the number of moles of $ClO^-$ are equal to the number of moles of KClO.

So, the number of moles of KClO = 0.0449 mole

Now we have to calculate the mass of KClO.

$\text{Mass of }KClO=\text{Moles of }KClO\times \text{Molar mass of }KClO$

$\text{Mass of }KClO=0.0449mole\times 90.6g/mole=4.07g\approx 4.1g$

Therefore, the mass of potassium hypochlorite is, 4.1 grams.

6 0

3 years ago

Which is a series circuit and a parallel circuit

kirza4 [7]

Explanation:

A is a series circuit

B is parallel circuit

8 0

3 years ago

Read 2 more answers

An isotope has three forms. 30% have a mass of 15 amu, 20% have a mass of 16 amu and 50% have a mass of 17 amu. What is the aver

murzikaleks [220]

Answer:

Explanation:

3 0

3 years ago

2. HBIO3 name this acid.

aleksandr82 [10.1K]

Answer:

Hydroxy(oxo)bismuthine oxide

3 0

3 years ago

Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those

Tanya [424]

Answer:

Q is 0.5 and K is 0.01, therefore K is less than Q.

the system will proceed in the reverse direction, thereby converting products into reactants. converting Nitric oxide to form oxygen and nitrogen.

Explanation:

Given,

N2 (g) + O2 (g) « 2 NO (g)

K = 0.01

heated temperature = 2000 ⁰C

N2 moles =0.4

O2 moles =0.1

2NO moles = 0.08

Volume of container = 1L

Q is the reaction quotient of the equilibrium equation. it is use to determined which direction the system will move to by comparing it with the K value.

Q can be calculated by multiplication of mass of reactant divide by mass of product

Q = $\frac{ [N2] *[O2}{2NO}$

the mass of the chemicals are in mole, there is need to convert them to moles/litre

therefore,

for N₂ : 0.4 mole per 1L container = 0.4 mol/L = 0.4M

for O₂ : 0.1 mole per 1L container = 0.1 mol/L = 0.1M

for 2NO : 0.08mole per 1L container = 0.08 mol/L = 0.08M

Q = $\frac{ [N2] *[O2}{2NO}$ = (0.4*0.1)/0.08 = 0.5

finally, we are going to compare the value of Q with K

Note that:

if K>Q , the reaction will proceed forward, converting reactants into product.

if K<Q , the reaction will proceed backward, converting products into reactants.

if K=Q , the system of reaction is already in equilibrium.

since, Q is 0.5 and K is 0.01, therefore K is less than Q.

the system will proceed in the reverse direction, thereby converting products into reactants. converting Nitric oxide to form oxygen and nitrogen.

7 0

3 years ago