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Stels [109]
3 years ago
9

How would you prepare a 1 L solution of 3 M MgO?

Chemistry
1 answer:
OleMash [197]3 years ago
8 0

Answer:

You need to measure 120.9132 grams of MgO and add to 1 liter of distilled water in a beaker.

Explanation:

Capital M stands for molarity, or moles/liter. So 3 M MgO means 3 moles per liter of MgO.

1 L × \frac{3 moles MgO}{1 L MgO} = 3 moles MgO

This means you need to measure 3 moles MgO to put into 1 Liter of water.

But you don't know how much that is, so you need to convert moles to grams.

First you need to find how many grams are in 1 mole of MgO.

You can search the molar mass of MgO online to get: 40.3044 g

But if you don't have the internet, use the periodic table to add the masses of Mg and O: 24.305 g + 15.999 g = 40.3044 g

Then write the fraction so that the units cancel out, so you get grams by itself on the top of the fraction.

1 L × \frac{3 moles MgO}{1 L MgO} × \frac{40.3044 g MgO}{1 mole MgO} = 120.9132 g MgO

You need to measure 120.9132 grams of MgO and add to 1 liter of distilled water.

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Answer:

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d. NaOH(aq) + HCl(aq) →  NaCl(aq) + H2O(1) COMBUSTION  REACTION.

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State and explain the relative change in the pH and in the buffer-component concentration ratio, [NaA]/[HA], for each of the fol
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When pure HA is added to the buffer, the buffer component ratio and the pH decrease.

<h3>State and explain the relative change in the pH and in the buffer-component concentration ratio, [NaA]/[HA] for the dissolve of pure HA in the buffer.</h3>

When pure HA is added to the buffer, the buffer component ratio and the pH decrease. The added HA increases the concentrations of NA and HA. However, there is a greater relative increase in the concentration of HA. Hence, the ratio of [NaA]/[HA] decreases, causing the solution to become more acidic.

The capacity of a buffer to withstand pH change is measured. The concentration of the buffer's components namely, the acid and its conjugate base determine this ability. Greater buffer capacity is associated with higher buffer concentration.

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A chemist heats the block of copper as shown in the interactive, then places the metal sample in a cup of oil at 25.00 °C instea
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When the oil is added to the heated copper, the energy in the system is

conserved.

  • The mass of the oil in the cup, is approximately <u>64.73 grams</u>.

Reasons:

The question parameters are;

Temperature of the oil in the cup = 25.00°C

Final temperature of the oil and copper, T₂ = 27.33 °C

Specific heat of copper, c₂ = 0.387 J/(g·°C)

Specific heat capacity of oil, c₁ = 1.74 J/(g·°C)

Required:

The<em> mass of oil</em> in the cup.

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The mass of the copper, m₂ = 17.920 g

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Therefore, we get;

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<em>The mass of the copper, m₂ = 17.920 g</em>

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