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Andre45 [30]
2 years ago
8

What is the act of adding fluid such as distilled water to a powdered or crystaline form?

Chemistry
1 answer:
nata0808 [166]2 years ago
6 0

Reconstitution is the act of adding fluid such as distilled water to a powdered or crystalline form.

Additionally, medications are frequently provided in dry form, such as powders or crystals, which must be reconstituted with liquid before being injected parenterally. To create a specified liquid concentration, a dry ingredient is reconstituted by adding a liquid diluent. To ensure that the drug is reconstituted in the exact concentration, it is crucial to carefully follow the reconstitution instructions. The quantity of fluid used to dilute the drug must also be taken into account when determining the dosage of reconstituted medication to provide to the patient.

Learn more about Reconstitution here-

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Calculate the ph of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions.
Makovka662 [10]

The pH of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions is 13.5.

<h3>What is pH? </h3>

pH is defined as the concentration of the hydrogen bond which is released or gained by the species in the solution which depicts the acidity and basicity of the solution.

<h3>What is pOH? </h3>

pOH is defined as the concentration of the hydronium ion present in solution.

pOH value is inversely proportional to the value of pH.

pH value increases, pOH value decreases and vice versa.

Given,

Total H+ ions = 2.95 ×10^(-12)M

<h3>Calculation of pH</h3>

pH = -log[H+]

By substituting the value of H+ ion in given equation

= log(2.95× 10^(-12) )

= 13.5

Thus we find that the pH of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions is 13.5.

learn more about pH:

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8 0
2 years ago
Aqueous sulfuric acid reacts with solid sodium hydroxide to produce aqueous sodium sulfate and liquid water. If 1.92 g of sodium
Oksana_A [137]

Answer:

The % yield is 27.0 %

Explanation:

<u>Step 1: </u>Data given

Mass of sulfuric acid = 4.9 grams

Mass of sodium hydroxide = 7.8 grams

Mass of sodium sulfate produced = 1.92 grams

Molar mass H2SO4 = 98.08 g/mol

Molar mass NaOH = 40 g/mol

Molar mass Na2SO4 = 142.04 g/mol

<u>Step 2: </u>The balanced equation

H2SO4 + 2NaOH → Na2SO4 + 2H2O

<u>Step 3</u>: Calculate moles H2SO4

Moles H2SO4 = Mass H2SO4 / Molar mass H2SO4

Moles H2SO4 = 4.9 grams / 98.08 g/mol =

Moles H2SO4 = 0.05 moles

<u>Step 4:</u> Calculate moles NaOH

Moles NaOH = 7.8 grams / 40 g/mol

Moles NaOH = 0.195 moles

<u>Step 5</u>: Calculate limiting reactant

For 1 mole H2SO4 consumed ,we need 2 moles NaOH to produce 1 mole Na2SO4 and 2 moles H2O

H2SO4 is the limiting reactant. It will completely be consumed (0.05 moles).

NaOH is in excess. There will react 2*0.05 = 0.1 moles

There will remain 0.195 -0.1 = 0.095 moles NaOH

<u>Step 6:</u> Calculate moles Na2SO4

For 1 mole H2SO4 consumed ,we need 2 moles NaOH to produce 1 mole Na2SO4

For 0.05 moles H2SO4, we have 0.05 moles Na2SO4

<u>Step 7:</u> Calculate mass of Na2SO4

Mass Na2SO4 = Moles Na2SO4 * Molar mass Na2SO4

Mass = 0.05 moles * 142.04 g/mol = 7.102

This is the theoretical yield

<u>Step 8:</u> Calculate the percent yield of Na2SO4

% yield = (actual yield / theoretical yield) * 100%

% yield = (1.92 /  7.102) *100% = 27.0 %

The % yield is 27.0 %

7 0
3 years ago
Explain why some metals are extracted by heating their oxides with carbon, but some metals cannot be extracted in this way
Oxana [17]

Answer:

This happens because a metal is less reactive than carbon and it can be extracted from its oxides by heating with carbon. The carbon displaces metal from the compound and removes the oxygen from the oxide.

8 0
3 years ago
During an experiment, a canister filled with hot water was added to a beaker filled with cold water. In which direction did the
Nady [450]

Answer:

A)

Explanation:

Heat moves from where it's hot, to where it's not

3 0
3 years ago
Để xác định hàm lượng Cu trong hợp kim Cu-Zn người ta làm như sau: Hòa
Goshia [24]
Answer: yes 1+1






Explain:
3 0
2 years ago
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