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ValentinkaMS [17]
3 years ago
7

A 1 liter solution contains 0.443 M acetic acid and 0.332 M sodium acetate. Addition of 0.365 moles of perchloric acid will: (As

sume that the volume does not change upon the addition of perchloric acid.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity
Chemistry
1 answer:
Yuki888 [10]3 years ago
4 0

Answer:

Lower the pH several units

Explanation:

Typically, a buffer system would minimize changes in pH values with additions of strong acid or base. However, one should realize buffer systems do have limits. The limits are dictated by the amount of common ion in the buffer solution mix. The chemistry of the buffer and common ion functions to remove the excess strong acid or base added. However, if more strong acid or strong base is added that exceeds the capacity of the buffer solution to remove the an excess acid or base solution would result and pH values would change drastically.

In this problem, perchloric acid (HClO₄) is a strong acid delivering hydronium ion in an amount equal to the amount of perchloric acid noted in the problem.

Since the concentration of perchloric acid (HClO₄) and H⁺ ion exceeds the concentration of available acetate ion in the buffer solution, the buffer effect would be exhausted before removing all of the HClO₄. The remaining HClO₄ would then function to drastically reduce the pH of the remaining solution several units before stabilizing.

The 0.443M HOAc/0.332M NaOAc buffer before addition of the HClO₄ has a pH of 4.62.  Adding 0.365M in HClO₄ would cause the HOAc equilibrium to shift left because of the H⁺ overload. This shift would continue until all of the strong acid was removed or all of the conjugate base is exhausted by converting back to HOAc. That is, adding 0.365M HClO₄ removes all 0.332M OAc⁻ leaving 0.365M - 0.332M = 0.033M excess HClO₄. The pH of a 0.033M HClO₄ solution => pH = -logs[H⁺] = -log(0.033) = 1.48.

=> compare pH before adding acid = 4.62 to pH after adding acid = 1.48.

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How many moles are in 2.5L of 1.75 M Na2CO3
mixas84 [53]

Answer: There are 4.375 moles in 2.5 L of 1.75 M Na_2CO_3

Explanation:

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}      

Molarity of solution = 1.75 M

Volume of solution = 2.5 L  

Putting values in equation , we get:

1.75M=\frac{\text{Moles of} Na_2CO_3}{2.5L}\\\\\text{Moles of }Na_2CO_3=1.75mol/L\times 2.5L=4.375mol

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3 years ago
At 20.°C, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0 milliliters of 1.0 M HCl(aq). Which change in conditions would
Pavlova-9 [17]

Answer: (2) decreasing the concentration of HCl(aq) to 0.1 M

Explanation: Rate of a reaction depends on following factors:

1. Size of the solute particles: If the reactant molecules are present in smaller size, surface of particles and decreasing the size increases the surface area of the solute particles. Hence, increasing the rate of a reaction.  

2. Reactant concentration: The rate of the reaction is directly proportional to the concentration of reactants.

3. Temperature: Increasing the temperature increases the energy of the molecules and thus more molecules can react to give products and rate increases.

(1) Increasing the initial temperature to 25°C will increase the reaction rate.

(2) Decreasing the concentration of HCl(aq) to 0.1 M will decrease the reaction rate due to lesser concentration.

(3) Using 1.2 g of powdered Mg will increase the reaction rate due to large surface area.

(4) Using 2.4 g of Mg ribbon will increase the reaction rate due to high concentration of reactants.

7 0
3 years ago
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Which states of matter change shape when moved? Which states of matter change shape when moved?
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Answer:

Gas and Liquids

Explanation:

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C12H22O11 + 11 H2SO4 12 C + 11 H2SO4 + 11 H2O
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Answer:

B: The sulfuric acid is not consumed or react with the reactant.

4 0
3 years ago
When 125 grams of FeO react with 25.0 grams of Al, how many grams of Fe can be produced? FeO + Al → Fe + Al2O3 25.9 g Fe 38.7 g
Serga [27]

<u>Answer:</u> The mass of iron produced will be 77.6 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

  • <u>For FeO:</u>

Given mass of FeO = 125 g

Molar mass of FeO = 71.8 g/mol

Putting values in equation 1, we get:

\text{Moles of FeO}=\frac{125g}{71.8g/mol}=1.74mol

  • <u>For aluminium:</u>

Given mass of aluminium = 25.0 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

\text{Moles of aluminium}=\frac{25.0g}{27g/mol}=0.93mol

The given chemical reaction follows:

3FeO+2Al\rightarrow 3Fe+Al_2O_3

By Stoichiometry of the reaction:

2 moles of aluminium metal reacts with 3 mole of FeO

So, 0.93 moles of aluminium metal will react with = \frac{3}{2}\times 0.93=1.395mol of FeO

As, given amount of FeO is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium metal is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of aluminium metal produces 3 mole of iron metal

So, 0.93 moles of aluminium metal will produce = \frac{3}{2}\times 0.93=1.395moles of iron metal

  • Now, calculating the mass of iron metal from equation 1, we get:

Molar mass of iron = 55.85 g/mol

Moles of iron = 1.395 moles

Putting values in equation 1, we get:

1.395mol=\frac{\text{Mass of iron}}{55.85g/mol}\\\\\text{Mass of iron}=(1.395mol\times 55.85g/mol)=77.6g

Hence, the mass of iron produced will be 77.6 grams

4 0
3 years ago
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