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4 years ago

Which of the following is a heterogeneous mixture?

Chemistry

2 answers:

sesenic [268]4 years ago

5 0

C because it is two seperate mixtures I think

IceJOKER [234]4 years ago

3 0

C. Oil and vinegar would be a heterogenous mixture.

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A leaf fell from a tree branch. The oath it followed is shown in the diagram below. Which of these best describes why the leaf f

andrey2020 [161]

Answer:

C-air currents and gravity applied changing and unbalanced forces to the leaf.

Explanation:

Dont trust me on this, but this is what I would choose!

I hope this helps!

8 0

3 years ago

Read 2 more answers

Chemistry: What is the result of heating copper carbonate? Thankyou x

Stels [109]

Answer:this is thermal decomposition

Explanation:

the light green copper carbonate when heated it gives copper oxide ( a black residue) and carbon dioxide is evolved

6 0

3 years ago

The metric unit for volume is the? A. pound B.quart C.liter D.gallon

Vladimir [108]

I believe it is liter.

5 0

4 years ago

Read 2 more answers

How many moles of Cu in 7.81 * 10^21 atoms of Cu

ICE Princess25 [194]

Use avogadro's number---> 6.02 x 10^23 atoms= 1 mol

7.81 x 10^21 (1 mole/ 6.02 x 10^23)= 0.0130 moles of Cu

8 0

3 years ago

As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the po

Ganezh [65]

Answer:

pH = 2.03

Explanation:

The pH can be calculated using the following equation:

$pH = -log [H_{3}O^{+}]$ (1)

The concentration of H₃O⁺ is calculated using the dissociation constant of the next reaction:

CH₃COOH + H₂O ⇄ CH₃COO⁻ + H₃O⁺

1.00 M

$K_{a} = \frac{[CH_{3}COO^{-}][H_{3}O^{+}]}{[CH_{3}COOH]}$

Solving the above equation for H₃O⁺, we have:

$[H_{3}O^{+}] = \frac{Ka*[CH_{3}COOH]}{[CH_{3}COO^{-}]}$ (2)

The dissociation constant is equal to:

$pKa = -log(Ka) \rightarrow Ka = 10^{-pKa} = 10^{-4.76} = 1.74 \cdot 10^{-5}$

Now, by solving the equation of the solubility product for Herbigon, we can find [CH₃COO⁻]:

CH₃COOX ⇄ CH₃COO⁻ + X⁺

5.00x10⁻³ M

$K_{sp} = [CH_{3}COO^{-}][X^{+}]$

$[CH_{3}COO^{-}] = \frac{K_{sp}}{[X^{+}]} = \frac{9.40 \cdot 10^{-6}}{5.00 \cdot 10^{-3}} = 1.88 \cdot 10^{-3} M$

By entering the values of [CH₃COO⁻] and Ka, into equation (2) we can calculate [H₃O⁺]:

$[H_{3}O^{+}] = \frac{1.74 \cdot 10^{-5}*[1.00]}{[1.88 \cdot 10^{-3}]} = 9.26 \cdot 10^{-3} M$

Hence, the pH is:

$pH = -log [H_{3}O^{+}] = -log [9.26 \cdot 10^{-3}] = 2.03$

Therefore, the pH must be 2.03 to yield a solution in which the concentration of X⁺ is 5.00x10⁻³M.

I hope it helps you!

6 0

4 years ago