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Maru [420]
2 years ago
10

A 25.00-ml sample of propionic acid, hc3h5o2, of unknown concentration was titrated with 0.141 m koh. the equivalence point was

reached when 37.48 ml of base had been added. what is the concentration of the propionate ion at the equivalence point?
a. 0.211 m
b. 0.147 m
c. 0.141 m
d. 0.0846 m
e. 0.128 m
Chemistry
1 answer:
Scorpion4ik [409]2 years ago
7 0
 The concentration of propionate ions   at  equivalent point is  0. 084 M
  calculation
write the equation for reaction
HC3H5O2   +  KOH  → H2O  + KC3H5O2

find the moles  of  KOH  used
moles=  molarity  × volume in liters
volume  in liters = 37.48 ml/1000 =0.03718L
molarity = 0.141 M


moles is therefore =  0.141 M  x0.03718 =  5.24238  x10^-3 moles

by use of mole  ratio between  KOH  and K3C3H5O2  which is 1:1  the  moles of K3C3H5O2  is also = 5.24238 x10^-3  moles

molarity is therefore = number  of moles/volume in liters
volume  in liters = 25/1000 +37.48/1000=0.06248 L

molarity of  propionate ions is therefore = (5.24238 x10^-3) / 0.06248 = 0.084  M
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4. A 14.5-L balloon is in the air where it is 20.0 C at 0.980-atm. A wind passes over and the balloon's pressure becomes 740.0-m
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The temperature of the wind as that decreases the volume and the pressure of the balloon to the given values is 14.09°C.

<h3>What is Combined gas law?</h3>

Combined gas law put together both Boyle's Law, Charles's Law, and Gay-Lussac's Law. It states that "the ratio of the product of volume and pressure and the absolute temperature of a gas is equal to a constant.

It is expressed as;

P₁V₁/T₁ = P₂V₂/T₂

Given the data in the question;

  • Initial volume V₁ = 14.5L
  • Initial pressure P₁ = 0.980atm
  • Initial temperature T₁ = 20.0°C = 293.15K
  • Final volume V₂ = 14.3L
  • Final pressure P₂ = 740.mmHg = 0.973684atm
  • Final temperature T₂ = ?

We substitute our given values into the expression above.

P₁V₁/T₁ = P₂V₂/T₂

( 0.980atm × 14.5L )/293.15K = ( 0.973684atm × 14.3L )/T₂

14.21Latm / 293.15K = 13.92368Latm / T₂

14.21Latm × T₂ = 13.92368Latm × 293.15K

14.21Latm × T₂ = 4081.72679LatmK

T₂ = 4081.72679LatmK / 14.21Latm

T₂ = 287.24K

T₂ = 14.09°C

Therefore, the temperature of the wind as that decreases the volume and the pressure of the balloon to the given values is 14.09°C.

Learn more about the combined gas law here: brainly.com/question/25944795

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