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Kaylis [27]
2 years ago
14

can someone please help me with this question, it's for my lab report. I tried my best but failed to do the calculation. please

it's an emergency, just do the best you can, even if you're not 100% sure with your answer, atleast it will give me an idea also where to start. Thank you

Chemistry
1 answer:
Dahasolnce [82]2 years ago
3 0

YOU BETTER MARK ME BRAINLIEST if someone else answers!!!!

When the two substances are mixed, we see an increase in the temperature,

The flat horizontal line at the beginning of the graph tells us the initial temperature of mixing the two substance.

The initial temperature of mixing is ≈22.5 oC

and, final temperature would be the next flat horizontal line ≈32.5 oC from the given graph

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24 because the sun has to be over his head again...?
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3 years ago
Consider the titration of a 20.0-mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each quantity. a. the initial pH b. t
Oksi-84 [34.3K]

Answer:

Explanation:

Given that:

Concentration of HC_2H_3O_2 \  (M_1) = 0.105 M

Volume of  HC_2H_3O_2 \  (V_1) = 20.0 mL

Concentration of NaOH (M_2) = 0.125 M

The  chemical reaction can be expressed as:

HC_2H_3O_2_{(aq)} + NaOH _{(aq)} \to NaC_2H_3O_2_{(aq)} + H_2O_{(l)}

Using the ICE Table to determine the equilibrium concentrations.

          HC_2 H_3 O_2 _{(aq)} + H_2O _{(l) } \to C_2 H_3O_2^- _{(aq)} + H_3O^+_{ (aq)}

I            0.105                                     0                  0

C              -x                                         +x                +x

E            0.105 - x                                  x                  x

K_a = \dfrac{[C_2H_5O^-_2][H_3O^+]}{[HC_2H_3O_2]}

K_a = \dfrac{(x)(x)}{(0.105-x)}

Recall that the ka for HC_2H_3O_2= 1.8 \times 10^{-5}

Then;

1.8 \times 10^{-5} = \dfrac{(x)(x)}{(0.105 -x)}

1.8 \times 10^{-5} = \dfrac{x^2}{(0.105 -x)}

By solving the above mathematical expression;

x = 0.00137 M

H_3O^+ = x = 0.00137  \ M \\ \\  pH = - log [H_3O^+]  \\ \\  pH = - log ( 0.00137 )

pH = 2.86

Hence, the initial pH = 2.86

b)  To determine the volume of the added base needed to reach the equivalence point by using the formula:

M_1 V_1 = M_2 V_2

V_2= \dfrac{M_1V_1}{M_2}

V_2= \dfrac{0.105 \ M \times 20.0 \ mL }{0.125 \ M}

V_2 = 16.8 mL

Thus, the volume of the added base needed to reach the equivalence point = 16.8 mL

c) when pH of 5.0 mL of the base is added.

The Initial moles of HC_2H_3O_2 = molarity × volume

= 0.105  \ M \times 20.0 \times 10^{-3} \ L

= 2.1 \times 10^{-3}

number of moles of 5.0 NaOH = molarity × volume

number of moles of 5.0 NaOH = 0.625 \times 10^{-3}

After reacting with 5.0 mL NaOH, the number of moles is as follows:

                    HC_2 H_3 O_2 _{(aq)} + NaOH _{(aq)} \to NaC_2H_3O_2_{(aq)} + H_2O{ (l)}

Initial moles   2.1*10^{-3}       0.625 * 10^{-3}           0                      0

F(moles) (2.1*10^{-3} - 0.625 \times 10^{-3})    0      0.625 \times 10^{-3}         0.625 \times 10^{-3}

The pH of the solution is then calculated as follows:

pH = pKa + log \dfrac{[base]} {[acid]}

Recall that:

pKa for HC_2H_3O_2=4.74

Then; we replace the concentration with the number of moles since the volume of acid and base are equal

∴

pH = 4.74 + log \dfrac{0.625 \times 10^{-3}}{1.475 \times 10^{-3}}

pH = 4.37

Thus, the pH of the solution after the addition of 5.0 mL of NaOH = 4.37

d)

We need to understand that the pH at 1/2 of the equivalence point is equal to the concentration of the base and the acid.

Therefore;

pH = pKa = 4.74

e) pH at the equivalence point.

Here, the pH of the solution is the result of the reaction in the (C_2H_3O^-_2) with H_2O

The total volume(V) of the solution = V(acid) + V(of the base added to reach equivalence point)

The total volume(V) of the solution = 20.0 mL + 16.8 mL

The total volume(V) of the solution = 36.8 mL

Concentration of (C_2H_3O^-_2) = moles/volume

= \dfrac{2.1 \times 10^{-3} \ moles}{0.0368 \ L}

= 0.0571 M

Now, using the ICE table to determine the concentration of H_3O^+;

             C_2H_5O^-_2 _{(aq)} + H_2O_{(l)} \to HC_2H_3O_2_{(aq)} + OH^-_{(aq)}

I              0.0571                                0                      0

C              -x                                       +x                     +x

E             0.0571 - x                             x                       x

Recall that the Ka for HC_2H_3O_2 = 1.8 \times 10^{-5}

K_b = \dfrac{K_w}{K_a} = \dfrac{1.0\times 10^{-14}}{1.8 \times 10^{-5} }  \\ \\ K_b = 5.6 \times 10^{-10}

k_b = \dfrac{[ HC_2H_3O_2] [OH^-]}{[C_2H_3O^-_2]}

5.6 \times 10^{-10} = \dfrac{x *x }{0.0571 -x}

x = [OH^-] = 5.6 \times 10^{-6} \ M

[H_3O^+] = \dfrac{1.0 \times 10^{-14} }{5.6 \times 10^{-6} }

[H_3O^+] =1.77 \times 10^{-9}

pH =-log  [H_3O^+]   \\ \\  pH =-log (1.77 \times 10^{-9}) \\ \\ \mathbf{pH = 8.75 }

Hence, the pH of the solution at equivalence point = 8.75

f) The pH after 5.09 mL base is added beyond (E) point.

             HC_2 H_3 O_2 _{(aq)} + NaOH _{(aq)} \to NaC_2H_3O_2_{(aq)} + H_2O{ (l)}

Before                             0.0021              0.002725         0

After                                   0                     0.000625        0.0021

[OH^-] = \dfrac{0.000625 \ moles}{(0.02 + 0.0218 )  \ L}

[OH^-] = \dfrac{0.000625 \ moles}{0.0418 \ L}

[OH^-] =  0.0149 \ M

From above; we can determine the concentration of H_3O^+ by using the following method:

[H_3O^+] = \dfrac{1.0 \times 10^{-14} }{0.0149}

[H_3O^+] = 6.7 \times 10^{-13}

pH = - log [H_3O^+]

pH = -log (6.7 \times 10^{-13} )

pH = 12.17

Finally, the pH of the solution after adding 5.0 mL of NaOH beyond (E) point = 12.17

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Two isotopes of the same element will have the same _____ but a different ____. (2 points)
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Two isotopes of the same element will have the same ATOMIC NUMBER but a different MASS NUMBER.

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Compute the equilibrium constant at 25 ∘C for the reaction between Sn2+(aq) and Cd(s), which form Sn(s) and Cd2+(aq). Express yo
Radda [10]

Answer:

6.1×10^8

Explanation:

The reaction is;

Sn^2+(aq) + Cd(s) -----> Sn(s) + Cd^2+(aq)

E°cell = E°cathode - E°anode

E°cathode= -0.14 V

E°anode= -0.40 V

E°cell = -0.14-(-0.40)

E°cell= -0.14+0.40

E°cell= 0.26 V

But

E°cell= 0.0592/n log K

E°cell= 0.0592/2 log K

0.26= 0.0296log K

log K = 0.26/0.0296

log K= 8.7838

K= Antilog (8.7838)

K= 6.1×10^8

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Which two systems first respond to burning your finger?
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Answer:

B. is my guess

I'm sorry if I'm wrong

God bless :)

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