Homework Answers
H2CO3 is diprotic acid but the second dissociation constant is very small, we can consider that H+ ions are mainly coming from the first dissociation of acid .
H2CO3
H+ + HCO3-
[H+] = √(c.Ka1) = √(0.10×4.3×10-7) = 2.0736×10-4 M
pH = -log[H+] = -log(2.0736×10-4) = 3.6833
pH = 3.68
Answer : (d) 3.68
Add Answer to:
What is the pH of a 0.10 M solution of carbonic acid? Carbonic acid, H2CO3 has...
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic...
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <->...
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.
1) Consider a 0.040 M solution of carbonic acid. Calculate the pH of this solution as well as the equilibrium concentra...
1) Consider a 0.040 M solution of carbonic acid. Calculate the pH of this solution as well as the equilibrium concentrations of: [H2CO3], [HCO3-], [H3O+], and [CO32-). H2CO3 + H20 5 HCO3 + H30+ K1 = 4.45 x 10-7 HCO3 + H20 5 CO32- + H30+ K2 = 4.69 x 10-11
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of...
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of CO3 -2. Ka1 = 4.30 x 10-7 Ka2 = 5.59 x 10-11
a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid...
a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid if the pH of this is 4.18. Ka1 (H2CO3) =4.45 x 10–7 and Ka2 =4.69 x 10–11 (b) Calculate the pH at the equivalence point of the titration between 0.1M CH3COOH (25 ml) with 0.05 M NaOH. Ka (CH3COOH) = 1.8 x 10–5.
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×...
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×10-7 and Ka2 = 5.6 × 10-11.10)A) 10.44 B) 5.50 C) 4.31 D) 11.00 E) 3.56
2. Calculate the pH of a 0.230 M calcium acetate solution if the Ka for acetic...
2. Calculate the pH of a 0.230 M calcium acetate solution if the Ka for acetic acid is 1.8x10-5 . 3. Calculate the pH of a 0.225 M solution of H2CO3. Ka1 = 4.3x10^-7 ; Ka2 = 5.6x10^-11 4. Calculate the pH of a 0.0080 M solution of sulfuric acid. Ka2 = 1.2x10^-2
Calculate the pH and concentration of species present in a polyprotic acid solution.
Calculate the pH and concentration of species present in a polyprotic acid solution.For a 3.44×10-3 M solution ofH2CO3, calculate both the pH and the CO32- ion concentration.H2CO3 + H2O → H3O+ +HCO3-Ka1 = 4.2×10-7HCO3- + H2O → H3O+ +CO32-Ka2 = 4.8×10-11pH =[CO32-] =
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 =...
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3]...
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.
1) Consider a 0.040 M solution of carbonic acid. Calculate the pH of this solution as well as the equilibrium concentrations of: [H2CO3], [HCO3-], [H3O+], and [CO32-). H2CO3 + H20 5 HCO3 + H30+ K1 = 4.45 x 10-7 HCO3 + H20 5 CO32- + H30+ K2 = 4.69 x 10-11
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?
Most questions answered within 3 hours.
-
An object in front of a concave mirror has a real image that is
11.5 cm...
asked 4 minutes ago -
Consider the reaction, C3 H8 + O2 --> CO2 + H2O. How many
moles of O2...
asked 1 hour ago -
You and your opponent both roll a fair die. If you both roll the
same number,...
asked 2 hours ago -
In a study of the accuracy of fast food drive-through orders,
Restaurant A had 257 accurate...
asked 2 hours ago -
Identify and describe in detail the four categories of
institutions that could be included in a...
asked 2 hours ago -
In python
class Customer:
def __init__(self, customer_id, last_name, first_name, phone_number, address):
self._customer_id = int(customer_id)
self._last_name =...
asked 2 hours ago -
What is an example of a limitation in implementing a new
ERP system and how it...
asked 2 hours ago -
In a section of 9.7cm of an artery with a radius of 2.6mm there
is a...
asked 2 hours ago -
the two carboxylic acid groups of aspartic acid have different
acidities with pKa values of 2.1...
asked 2 hours ago -
Would CuCO3 aqueous salt combined with calcium chloride
form a solid precipitate? If so, what would...
asked 2 hours ago -
How do ECM Solutions assist in embedding a culture of continuous
improvement in an organization? (Project...
asked 2 hours ago -
Directions
These directions introduce the idea of Essential Questions.
Since this may be a new concept...
asked 2 hours ago