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gregori [183]
2 years ago
11

Plzzzz help due in like 10 min!!!

Chemistry
2 answers:
muminat2 years ago
3 0

Answer: for question 4, the answer would most likely be movement of air, water and rock

Explanation:

o-na [289]2 years ago
3 0

Answer:

Explanation:

<em>It is really blurry i cant really see the pic</em>

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What is the number of moles of NaOH in 16.5 mL of 0.750 Molar NaOH?
Alchen [17]

Answer:

0.0165 (L) * 0.750 (mol/L) = 0.0124 mol NaOH in 16.5 mL

Explanation:

5 0
2 years ago
WILL GIVE BRAINLIEST AND 5 STARS what is the purpose/ use of a Bunsen Burner
Roman55 [17]

A Bunsen burner, named after Robert Bunsen, is a common piece of laboratory equipment that produces a single open gas flame, which is used for heating, sterilization, and combustion. The gas can be natural gas (which is mainly methane) or a liquefied petroleum gas, such as propane, butane, or a mixture of both. Have A Great Day :)

5 0
3 years ago
Read 2 more answers
How does weathering change rock and minerals
Phantasy [73]

Weathering is the process of breaking large rocks and boulders into much smaller ones. Weathering can be brought about by wind and water mostly. Sometimes even biological forces account for some types of weathering.

3 0
3 years ago
Read 2 more answers
Which of the following is an example of a nonmetal that is solid at room
Darya [45]

Answer:

Carbon

Explanation:

At room temperature20–22 °C (68–72 °F), nitrogen and oxygen are gases, while bromine is a liquid.

6 0
2 years ago
In an aqueous solution of a certain acid the acid is 4.4% dissociated and the pH is 3.03. Calculate the acid dissociation consta
NeX [460]

Answer:

4.1x10⁻⁵

Explanation:

The dissociation of an acid is a reversible reaction, and, because of that, it has an equilibrium constant, Ka. For a generic acid (HA), the dissociation happens by:

HA ⇄ H⁺ + A⁻

So, if x moles of the acid dissociates, x moles of H⁺ and x moles of A⁻ is formed. the percent of dissociation of the acid is:

% = (dissociated/total)*100%

4.4% = (x/[HA])*100%

But x = [A⁻], so:

[A⁻]/[HA] = 0.044

The pH of the acid can be calcualted by the Handersson-Halsebach equation:

pH = pKa + log[A⁻]/[HA]

3.03 = pKa + log 0.044

pKa = 3.03 - log 0.044

pKa = 4.39

pKa = -logKa

logKa = -pKa

Ka = 10^{-pKa}

Ka = 10^{-4.39}

Ka = 4.1x10⁻⁵

4 0
3 years ago
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