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3 years ago

Write about buffer solution with its formulas

Chemistry

1 answer:

musickatia [10]3 years ago

8 0

Answer:

A buffer solution is a mixture of two pair salts to maintain a stable pH.

Explanation:

This mixture is made always with a complementary pair of salts (one acid an another basic).

Example:

Acetic Acid (CH3COOH) and Sodium Acetate (NaH3COO).

So when you add a little bit more acid to this mixture, the basic part of the buffer, in this case the Sodium Acetate, will neutralize it and the pH will remain the same.

On the other hand, if the mixture receives some basic substance, the acid part of the buffer, the acetic acid, will neutralize it, so again the pH will remain the same.

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How many elements and how many atoms are in MgCI2

aliina [53]

Answer: two elements and three atoms

Explanation:

An element is the simplest substance and hence cannot be broken down using chemical reactions.

Magnesium chloride $(MgCl_2)$ is an ionic compound formed by the transfer of electrons from element magnesium (Mg) to element chlorine (Cl) where Magmesium forms a cation $Mg^{2+}$ by losing two electrons and chlorine forms an anion $Cl^{-}$ by gaining electron.

There are 3 atoms in Magnesium chloride $(MgCl_2)$ which include one atom of magnesium (Mg) and two atoms of chlorine (Cl).

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3 years ago

Using the van der waals equation, the pressure in a 22.4 l vessel containing 1.50 mol of chlorine gas at 0.00 °c is ________ atm

Lana71 [14]

Answer is: the pressure in a vessel is 1.48 atm.

V(Cl₂) = 22.4 L; pressure of chlorine gas.

n(Cl₂) = 1.50 mol; amount of chlorine gas.

T = 0.00°C = 273.15 K; temperature.

a = 6.49 L²·atm/mol²; the constant a provides a correction for the intermolecular forces.

b = 0.0562 L/mol; value is the volume of one mole of the chlorine gas.

R = 0.08206 L·atm/mol·K, universal gas constant.

Van de Waals equation: (P + an² / V²)(V - nb) = nRT.

(P + 6.49 L²·atm/mol² · (1.5 mol)² / (22.4 L)²) · (22.4 L - 1.5 mol·0.0562 L/mol) = 1.5 mol · 0.08206 L·atm/mol·K · 273.15 K.

(P + 6.49 L²·atm/mol² · (1.5 mol)² / (22.4 L)²) = (1.5 mol · 0.08206 L·atm/mol·K · 273.15 K) ÷ (22.4 L - 1.5 mol · 0.0562 L/mol).

P + 0.029 atm = 33.62 L·atm ÷ 22.31 L.

P = 1.507 atm - 0.029 atm.

P = 1.48 atm; the pressure.

7 0

3 years ago

What is the molar mass of Na(C2 H3 O2)?

Lunna [17]

The molar mass of this equation is 98.04

5 0

3 years ago

Read 2 more answers

Help me pleaseeee, ty if you doo:))

allochka39001 [22]

Answer:

9 is the correct answer

4 0

3 years ago

A chemist adds of a sodium thiosulfate solution to a reaction flask. Calculate the mass in grams of sodium thiosulfate the chemi

schepotkina [342]

This is a incomplete question.The complete question is:

A chemist adds 180.0 ml of a 1.77 mol/L of sodium thiosulfate solution to a reaction flask. Calculate the mass in grams of sodium thiosulfate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Answer: 50.4 g

Explanation:

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

$\text{Moles of solute}={\text{Molarity of the solution}}\times{\text{Volume of solution (in L)}}$ .....(1)

Molarity of sodium thiosulfate solution = 1.77 M

Volume of sodium thiosulfate solution = 180.0 mL = 0.1800 L

Putting values in equation 1, we get:

$\text{Moles of sodium thiosulfate}={1.77}\times{0.1800}=0.319moles$

Mass of sodium thiosulfate = $moles\times {\text {Molar mass}}=0.319moles\times 158.11g/mol=50.4g$

Thus 50.4 g of sodium thiosulfate the chemist has added to the flask.

6 0

3 years ago

Write about buffer solution with its formulas​

Write about buffer solution with its formulas