Answers
Answer:
pH of Buffer Solution 5.69
Explanation:
Mole of anhydrous sodium acetate =
=
= 0.18 mole
100 ml of 0.2 molar acetic acid means
= M x V
= 0.2 x 100
= 20 mmol
= 0.02 mole
Using Henderson equation to find pH of Buffer solution
pH = pKa + log
= 4.74 + log
= 4.74 + log 9
= 5.69
So pH of the Buffer solution = 5.69
Related Questions
Which beat describes heat
What data should be plotted to show that experimental concentration data fits a first-order reaction? A) 1/[reactant] vs. time B) [reactant) vs. time C) In[reactant] vs. time D) In(k) vs. 1/1
Hi ! Could someone help me out with this last part to my chemistry practice ? Thank you !
Suppose one was doing this experiment in the real world and the stockroom ran out of NaCl solutions. Which other solutions of similar concentration could be used in place of NaCl(aq)
i. two
ii. three
iii. six
iv. eight
(b) How many atoms are directly bonded to the central atom in a trigonal bipyramidal molecule?
i. three
ii. four
iii. five
iv. six
(c) How many atoms are directly bonded to the central atom in an octahedral molecule?
i. three
ii. four
iii. six
iv. eight
Answers
Answer:
a) ii
b)iii
c)iii
Explanation:
three atoms directly bonded then only it is possible to achieve trigonal planar
trigonal bipyramidal means five atoms should attach to central atom
for octahedral six atoms must directly connected to central atom
Answers
Answer
Naphthalene is a non electrolyte
If the unknown compound is an electrolyte it gives 2 or more ions in solution
( NaCl >> Na+ + Cl- => 2 ions
Ca(NO3)2 >> Ca2+ + 2 NO3- => 3 ions)
the f.p. lowering is directly proportional to the molal concentration of dissolved ions in the solution )
For naphthalene
delta T = 1.86 x m
for a salt that gives 2 ions
delta T = 1.86 x m x 2
hence the lowering in freezion point of unkown is greater then napthalene
They live in water,
B
They are cold blooded,
С
They do not have scales,
D
They do not have backbones,
Answers
Answers
Answer:
Explanation:
Hello,
Considering the given reaction's stoichiometry, grams of oxygen result:
Moreover, the mass of produced carbon dioxide turns out:
Best regards.
Answers
Answer: The pH of the buffer is 4.61
Explanation:
To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:
We are given:
= negative logarithm of acid dissociation constant of weak acid = 4.70
= moles of conjugate base = 3.25 moles
= Moles of acid = 4.00 moles
pH = ?
Putting values in above equation, we get:
Hence, the pH of the buffer is 4.61
(c) Why might the suggestion for part (b) be of benefit to middle-distance runners?
Answers
Answer:
a) [HCO₃⁻] = 10,2 mM.
b) Sodium bicarbonate.
c) Yes.
Explanation:
a) The equilibrium of this reaction is:
CO₂ + H₂O ⇄ HCO₃⁻ + H⁺
Using Henderson-Hasselbalch equation:
pH = pka + log₁₀
Replacing:
7,03 = 6,1 + log₁₀
Thus, [HCO₃⁻] = 10,2 mM
b) A possible treatment of metabolic acidosis is with sodium bicarbonate. By Le Chateleir's principle the increasing of HCO₃⁻ will shift the equilibrium to the left decreasing thus, H⁺ concentration.
c) The shifting of the equilibrium to the left will increase CO₂ concentration producing in the body the need to increase breathing, increasing, thus, concentration of O₂ improving cardiac function in exercise.