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aleksley [76]
4 years ago
13

What is potential energy?

Chemistry
2 answers:
V125BC [204]4 years ago
4 0

The energy possessed by a body by virtue of its position relative to others, stresses within itself, electric charge, and other factors.

Helga [31]4 years ago
4 0

Answer:

\boxed{\mathrm{view \ explanation}}

Explanation:

Potential energy is the energy stored in a body due to the body’s positioning or state.

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The chemistry of anhydrides is similar to that of acid chlorides, although they react more slowly.
Volgvan

Answer:

both

Explanation:

6 0
3 years ago
A 5.00g quantity of a diprotic acid was dissolved in water and made up exactly 250 mL. Calculate the molar mass if the acid is 2
MAXImum [283]

Answer:

The molar mass of the diprotic acid is 90.10 g/mol.

Explanation:

The acid is 25.0 mL of this solution required 11.1 mL of 1.00 KOH for neutralization.

H_2A+2KOH\rightarrow K_2A+2H_2O

To calculate the concentration of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2  ( neutralization )

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of diprotic acid

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is KOH.

We are given:

n_1=2\\M_1=?\\V_1=25 mL\\n_2=1\\M_2=1.00 M\\V_2=11.1 mL

Putting values in above equation, we get:

2\times M_1\times 25=1\times 1.00\times 11.1}

M_1=\frac{1\times 1.00\times 11.1}{2\times 25}=0.222 M

Molarity of acid solution = 0.222 M =0.222 mol/L

Volume of original solution = 250 mL = 0.250 L ( 1 mL = 0.001 L)

Moles of diprotic acid in 0.250 L solution :

=0.222 mol/L\times 0.250 L=0.0555 mol

Mass of diprotic acid = m = 5.00 g

Moles(n)=\frac{mass(m)}{\text{Molar mass(M)}}

M=\frac{m}{n}=\frac{5.00 g}{0.0555 mol}=90.10 g/mol

The molar mass of the diprotic acid is 90.10 g/mol.

5 0
3 years ago
A crystalline solid has a high melting point and is known to be held together with covalent bonds. This solid is an example of _
OverLord2011 [107]
Letter B is correct the answer
5 0
4 years ago
In standardizing the solution of aqueous sodium hydroxide, a chemist overshoots the end point and adds too much naoh(aq). would
irinina [24]

Answer: Concentration of NaOH calculated will be underestimated.

Explanation:

End point is an observational point , which tells us about the completion of reaction between the titrant (solution in burette) and titre(solution in conical flask) in titration experiment.

In this case , NaOH is titrant whose concentration is unknown.

M_1=\text{molarity of titre} , M_2=\text{molarity of NaOH}

V_1=\text{volume of titre} , V_2=\text{volume of NaOH}

M_1V_1=M_2V_2

M_2=\frac{M_1V_1}{V_2}....(1)

According to question a chemist overshoots the end point and adds to much of NaOH solution, which means increase in the value of V_2.

Then the value of M_2 in equation (1), will get lowered , which means that the concentration of NaOH was lower than that of the actual value. Hence underestimated concentration of NaOH.




8 0
3 years ago
Potassium hydroxide is very soluble in water, resulting in extremely basic solutions. A 121g sample KOH is dissolved in water at
nataly862011 [7]

Answer:

15.33

Explanation:

Given parameters:

Mass of KOH = 121g

Volume of solution  = 100mL   = 0.1dm³

Molar mass of KOH  = 56.11g/mol

Unknown:

pH  of the solution = ?

Solution:

To find the pH, we must first know the concentration of the solution obtained by mixing KOH up to this volume.

This can be done by finding the molarity of the solution.

  Molarity  = \frac{number of moles }{volume of solution}

  Number of moles of KOH  = \frac{mass}{molar mass}    = \frac{121}{56.11}   = 2.16mole

Input parameters;

 Molarity of solution = \frac{2.16}{0.1}   = 21.6moldm⁻³

       KOH    →    OH⁻   +          K⁺

       21.6           21.6              21.6

In the solution we have 21.6moldm⁻³ of OH⁻ which is need to find the pH;

          pOH  = -log₁₀(OH⁻)

         pOH  =  -log₁₀21.6

          pOH  = -1.33

Since pH + pOH   = 14

          pH  = 14 - (-1.33)  = 15.33

3 0
4 years ago
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