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Nutka1998 [239]
2 years ago
11

Phosphate buffers are commonly used in biological research. If a small amount of strong acid is added to a buffer solution that

is 0.700 M H3PO4 and 0.700 M KH2PO4, which of the following statements is true?
A) [H3PO4] will increase, [KH2PO4] will decrease, and pH will slightly decrease.
B) [H3PO4] will increase, [KH2PO4] will decrease, and pH will not change.
C) [H3PO4] will decrease, [KH2PO4] will increase, and pH will slightly decrease.
D) [H3PO4] will decrease, [KH2PO4] will increase, and pH will slightly increase.
E) [H3PO4] will increase, [KH2PO4] will decrease, and pH will slightly increase.
F) [H3PO4] will decrease, [KH2PO4] will increase, and pH will not change
Chemistry
1 answer:
lozanna [386]2 years ago
4 0

Answer:

A) [H3PO4] will increase, [KH2PO4] will decrease, and pH will slightly decrease.

Explanation:

A buffer is a solution which resists changes to its pH when a small amount of acid or base is added to it.

Buffers consist of a weak acid (HA) and its conjugate base (A–) or a weak base and its conjugate acid. Weak acids and bases do not completely dissociate in water, and instead exist in solution as an equilibrium of dissociated and undissociated species. When a small quantity of a strong acid is added to a buffer solution, the conjugate base, A-, reacts with the hydrogen ions from the added acid to form the weak acid and a salt thereby removing the extra hydrogen ions from the solution and keeping the pH of the solution fairly constant. On the other hand, if a small quantity of a strong base is added to the buffer solution, the weak acid dissociates further to release hydrogen ions which then react with the hydroxide ions of the added base to form water and the conjugate base.

For example, if a small amount of strong acid is added to a buffer solution that is 0.700 M H3PO4 and 0.700 M KH2PO4, the following reaction is obtained:

KH₂PO₄ + H+ ----> K+ + H₃PO₄

Therefore, [H₃PO₄] will increase, [KH₂PO₄] will decrease, and pH will slightly decrease.:

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Two different compounds are formed by the elements nitrogen and oxygen. The first compound, compound P1, contains 64.17% by mass
xz_007 [3.2K]

Answer:

Explanation:

To solve the problem, we must know the kind of compounds we are dealing with.

For the first compound, P1 and second compound P2:

                                N                       O                         N                     O

Mass percent       64.17                 35.73                  47.23               52.79

Atomic mass          14                      16                         14                    16

Number of

moles            64.17/14            35.73/16            47.23/14    52.79/16      

                            4.58                  2.23                     3.37                  3.30

Simplest

ratio                 4.58/2.23            2.23/2.23             3.37/3.30         3.3/3.3

                              2                           1                             1                        1

                             

P1 compound is N₂O

P2 compound is NO

These are the compounds,

   In N₂O = 28:16

          NO = 14:16

This is the ratio of nitrogen to a fixed mass of oxygen for the two compounds.

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I hope that made sense.
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Answer:

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3 years ago
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VARVARA [1.3K]

Answer:

This is a pretty straightforward example of how an ideal gas law problem looks like.

Your strategy here will be to use the ideal gas law to find the pressure of the gas, but not before making sure that the units given to you match those used by the universal gas constant.

So, the ideal gas law equation looks like this

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

P

V

=

n

R

T

a

a

∣

∣

−−−−−−−−−−−−−−−

Here you have

P

- the pressure of the gas

V

- the volume it occupies

n

- the number of moles of gas

R

- the universal gas constant, usually given as

0.0821

atm

⋅

L

mol

⋅

K

T

- the absolute temperature of the gas

Take a look at the units given to you for the volume and temperature of the gas and compare them with the ones used in the expression of

R

.

a

a

a

a

a

a

a

a

a

a

a

Need

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

Have

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

a

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a

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a

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a

a

a

a

a

a

a

a

a

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a

a

a

a

a

a

a

a

a

a

Liters, L

a

a

a

a

a

a

a

a

a

a

a

a

a

Liters, L

a

a

a

a

a

a

a

a

a

a

a

√

a

a

a

a

a

a

a

Kelvin, K

a

a

a

a

a

a

a

a

a

a

a

a

Celsius,

∘

C

a

a

a

a

a

a

a

a

a

×

Notice that the temperature of the gas must be expressed in Kelvin in order to work, so make sure that you convert it before plugging it into the ideal gas law equation

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

T

[

K

]

=

t

[

∘

C

]

+

273.15

a

a

∣

∣

−−−−−−−−−−−−−−−−−−−−−−−−

Rearrange the ideal gas law equation to solve for

P

P

V

=

n

R

T

⇒

P

=

n

R

T

V

Plug in your values to find

P

=

0.325

moles

⋅

0.0821

atm

⋅

L

mol

⋅

K

⋅

(

35

+

273.15

)

K

4.08

L

P

=

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

2.0 atm

a

a

∣

∣

−−−−−−−−−−−

The answer is rounded to two sig figs, the number of sig figs you have for the temperature of the gas.

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