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ss7ja [257]
3 years ago
15

What is the % by volume of 50mL of ethylene glycol dissolved in 950mL of H2O?

Chemistry
1 answer:
MariettaO [177]3 years ago
5 0

Answer:

5.0 %

Explanation:

Given data

  • Volume of ethylene glycol (solute): 50 mL
  • Volume of water (solvent): 950 mL

Step 1: Calculate the volume of solution

If we assume that <em>the volumes are additive</em>, the volume of the solution is equal to the sum of the volume of the solute and the solvent.

V = 50 mL + 950 mL = 1000 mL

Step 2: Calculate the percent by volume

We will use the following expression.

\% v/v = \frac{volume\ of\ solute}{volume\ of\ solution} \times 100 \%  = \frac{50mL}{1000mL} \times 100 \% = 5.0\%

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Please help me with number 4 and 5 on my study guide
Shtirlitz [24]

Answer:

help with problem 4

Explanation:

4. protons are equal to atomic numbers. neutrons are atomic mass minus atomic number. electrons are equal to protons.

5. I don't know, sorry.

5 0
2 years ago
Consider the following equilibrium:
Ainat [17]

<u>Answer: </u>The equation which is wrong is K_p=K_c(RT)^{-5}

<u>Explanation:</u>

For the given reaction:

4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)

The expression for K_c\text{ and }K_p is given by:

K_c=\frac{1}{[O_2]^3}

K_p=\frac{1}{[O_2]^3}

The concentration of solids are taken to be 1, only concentration of gases and liquid states are taken. The pressure of only gases are taken.

Relationship between K_p\text{ and }K_c is given by the expression:

K_p=K_c\times (RT)^{\Delta n_g}

where,

\Delta n_g= number of moles of gaseous products - number of moles of gaseous reactants

R = gas constant

T= temperature

For the above reaction,

\Delta n_g = number of moles of gaseous products - number of moles of gaseous reactants = 0 - 3 = -3

Hence, the expression for K_p is:

K_p=K_c\times (RT)^{-3}

Therefore, the equation which is wrong is K_p=K_c(RT)^{-5}

7 0
3 years ago
Why is the bond between two single hydrogen atoms stable?
Len [333]
B ia the correct one .

Hydrogen only uses the first energy shell, which holds 2 electrons, not 8.
5 0
3 years ago
Read 2 more answers
Please answer with an actual answer and not just put a random word ^-^
WARRIOR [948]

Which eclipse was modeled when the large ball was between the small ball and the light?

The model is a "Lunar Eclipse" (If it was talking about the earth, then yes, it is a lunar eclipse).

<u>                                                               </u>

Which eclipse was modeled when the small ball was between the large ball and the light?

The model is a "Solar Eclipse".

<u>                                                               </u>

What does the large ball represent?

The earth.

<u>                                                               </u>

What does the small ball represent?

The moon.

<u>                                                               </u>

What does the light source represent?

The sun.

Hope this helps!~ <3

(I can't draw so sorry.)

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6 0
3 years ago
Calculate the ph of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pka ???? 4.76) of (a) 2:1
givi [52]

According to Hasselbach-Henderson equation:

pH=pK_{a}+log\frac{[A^{-}]}{[HA]}

Here, [A^{-}] is concentration of conjugate base and [HA] is concentration of acid.

In the given problem, conjugate base is CH_{3}COOK and acid is CH_{3}COOH thus, Hasselbach-Henderson equation will be as follows:

pH=pK_{a}+log\frac{[CH_{3}COOK]}{[CH_{3}COOH]}...... (1)

(a) Ratio of concentration of potassium acetate and acetic acid is 2:1 thus,

\frac{[CH_{3}COOK]}{[CH_{3}COOH]}=2

Also, pK_{a}=4.76

Putting the values in equation (1),

pH=4.76+log\frac{2}{1}=5.06

Therefore, pH of solution is 5.06.

(b) Ratio of concentration of potassium acetate and acetic acid is 1:3 thus,

\frac{[CH_{3}COOK]}{[CH_{3}COOH]}=\frac{1}{3}

Also, pK_{a}=4.76

Putting the values in equation (1),

pH=4.76+log\frac{1}{3}=4.28

Therefore, pH of solution is 4.28.

(c)Ratio of concentration of potassium acetate and acetic acid is 5:1 thus,

\frac{[CH_{3}COOK]}{[CH_{3}COOH]}=\frac{5}{1}

Also, pK_{a}=4.76

Putting the values in equation (1),

pH=4.76+log\frac{5}{1}=5.45

Therefore, pH of solution is 5.45.

(d) Ratio of concentration of potassium acetate and acetic acid is 1:1 thus,

\frac{[CH_{3}COOK]}{[CH_{3}COOH]}=1

Also, pK_{a}=4.76

Putting the values in equation (1),

pH=4.76+log\frac{1}{1}=4.76

Therefore, pH of solution is 4.76.

(e) Ratio of concentration of potassium acetate and acetic acid is 1:10 thus,

\frac{[CH_{3}COOK]}{[CH_{3}COOH]}=\frac{1}{10}

Also, pK_{a}=4.76

Putting the values in equation (1),

pH=4.76+log\frac{1}{10}=3.76

Therefore, pH of solution is 3.76.

4 0
3 years ago
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