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Illusion [34]
2 years ago
15

You removed a Coke can from the refrigerator. When you come back a few minutes later, you realize the can has begun to "sweat".

Chemistry
1 answer:
Vinvika [58]2 years ago
8 0

Answer:

B

Explanation:

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Calcium carbonate is often used as an antacid. Your stomach acid is composed of HCl at a pH of 1.5. If you ate toooo much Turkey
stiks02 [169]

<u>Answer:</u> 0.0237 g of calcium carbonate would be required to neutralize the given amount of HCl

<u>Explanation:</u>

pH is defined as the negative logarithm of hydrogen ion concentration present in the solution

pH=-\log [H^+]      .....(1)

Given value of pH = 1.5

Putting values in equation 1:

1.5=-\log[H^+]

[H^+]=10^{(-1.5)}=0.0316M

Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:

\text{Molarity of solution}=\frac{\text{Number of moles of solute}\times 1000}{\text{Volume of solution (mL)}}       .....(2)

We are given:

Volume of solution = 15.0 mL

Molarity of HCl = 0.0316 M

Putting values in equation 2:

0.0316=\frac{\text{Moles of HCl}\times 1000}{15.0}\\\\\text{Moles of HCl}=\frac{0.0316\times 15.0}{1000}=4.74\times 10^{-4}mol

The chemical equation for the reaction of HCl and calcium carbonate follows:

2HCl+CaCO_3\rightarrow H_2CO_3+CaCl_2

By the stoichiometry of the reaction:

2 moles of HCl reacts with 1 mole of calcium carbonate

So, 4.74\times 10^{-4}mol of HCl will react with = \frac{1}{2}\times 4.74\times 10^{-4}=2.37\times 10^{-4}mol of calcium carbonate

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of calcium carbonate = 2.37\times 10^{-4}mol

Molar mass of calcium carbonate = 100.01 g/mol

Putting values in the above equation:

\text{Mass of }CaCO_3=(2.37\times 10^{-4}mol)\times 100.01g/mol\\\\\text{Mass of }CaCO_3=0.0237g

Hence, 0.0237 g of calcium carbonate would be required to neutralize the given amount of HCl

7 0
2 years ago
Which of the following would make a solution?
gizmo_the_mogwai [7]

Answer:

B sugar in water

Explanation:

because sugar dissolves in water while the others don't

8 0
2 years ago
Read 2 more answers
What do elements Be,Mg,Ca have in common
Strike441 [17]
They are all in the same family
5 0
3 years ago
Read 2 more answers
How do you think the amount of a material affects its tendency to sink or float? <br> ASAP
Ksivusya [100]

Answer:

it dependes on the material

Explanation:

what is the material

3 0
3 years ago
Write the formula for potassium oxide. why do you not need prefixes in the name ​
Molodets [167]

Potassium oxide: K₂O.

There's no need for prefixes since K₂O is an ionic compound.

<h3>Explanation</h3>

Find the two elements on a periodic table:

  • Potassium- K- on the left end of period four.
  • Oxygen- O- near the right end of periodic two.

Elements on the bottom-left corner of the periodic table are metals. Those on the top-right corner are nonmetals.

  • Potassium is a metal,
  • Oxygen is a nonmetal.

A metal and a nonmetal combine to form an ionic compound. Potassium oxide is likely to be an ionic compound. It contains two types of ions:

  • Potassium ions: Potassium is group 1 of the periodic table. It is an alkaline metal. Like other alkaline metals such as sodium Na, potassium K tends to lose one electron and form ions of charge +1 in compounds. The ion would be K⁺.
  • Oxide ions from oxygen: Oxygen is the second most electronegative element on the periodic table. It tends to gain two electrons and form the oxide ion \text{O}^{2-} when it combines with metals.

The two types of ions carry opposite charges. They shall pair up at a certain ratio such that they balance the charge on each other. The charge on each \text{O}^{2-} ion is twice that on a \text{K}^{+} ion. Each \text{K}^{+} would pair up with two \text{O}^{2-}. Hence the subscript in the formula: \text{K}_{\bf 2}\text{O}.

There are two classes of compounds:

  • Covalent compounds, which need prefixes, and
  • Ionic compounds, which need no prefix.

Prefixes are needed only in covalent compounds. For instance in the covalent compound carbon dioxide \text{CO}_2, the prefix di- indicates that there are two oxygen atoms in the formula \text{CO}_2. However, there's no need for prefix in ionic compounds such as \text{K}_2\text{O}.

7 0
3 years ago
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