If a buffer solution is 0.100 M in a weak acid (K, = 5.7 x 10-5) and 0.530 M in its conjugate base, what is the pH? pH =

Q: If a buffer solution is 0.230 M in a weak acid (Ka = 3.4 x 10-3) and 0.410 M in its conjugate base,…

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Q: If a buffer solution is 0.120 M in a weak acid (Ka = 5.4 x 10-) and 0.480 M in its conjugate base,…

A:

Q: HCIO is a weak acid (Ka = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Ka of HClO = 4.0 × 10-8 Concentration of the solution of NaClO = 0.089 M pH =?

Q: If a buffer solution is 0.170 M in a weak base (Kb = 4.2 × 10-5) and 0.490 M in its conjugate acid,…

A: Buffer solution: It is an aqueous solution which contains a mixture of a weak base and its conjugate…

Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: If the Kp of a weak base is 3.4 × 10-0, what is the pH of a 0.25 M solution of this base? pH =

A:

Q: If a buffer solution is 0.110 M in a weak base (K, = 1.9 × 10-³) and 0.480 M in its conjugate acid,…

A: Given that:  [Base] = 0.110M  [Salt] = 0.480M  Kb = 1.9×10-5 Pkb = -logKb = -log(1.9×10-5) = 4.72…

Q: What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.47 M in HIO? The Ka for HIO is 2.3…

A: When a weak acid(eg HIO) mixed with its conjugate base (ege IO-) they form a buffer solution. pH of…

Q: A solution is prepared that is initially 0.0010 M NaOH and 0.10 M NH3. What is the pH of this…

A: [NaOH] =0.001 M [NH3] = 0.10M

Q: A students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH…

A:

Q: If a buffer solution is 0.280 M in a weak base (K, = 5.7 x 10-5) and 0.450 M in its conjugate acid,…

A: We have to predict the pH of the solution.

Q: What is the pH of a solution containing 0.225 M weak base, B', with a K, of 3.8 X 10-7? в (аq) + Н,О…

A:

Q: If a buffer solution is 0.260 M in a weak base (Kp = 1.4 x 10-5) and 0.560 M in its conjugate acid,…

A: Answer: pH = 8.8125

Q: If a buffer solution is 0.150 M in a weak base (K, = 3.5 × 10-5) and 0.430 M in its conjugate acid,…

A: The Henderson- Hasselbalch equation can be used for the for the evaluation of pOH of the buffer…

Q: If a buffer solution is 0.160 M in a weak acid (Ka = 2.1 × 10-5) and 0.580 M in its conjugate base,…

A: The question is about calculating the pH of a buffer solution with the given data -

Q: If a buffer solution is 0.170 M in a weak base (?b=3.7×10−5) and 0.540 M in its conjugate acid, what…

A: In question it is not mentioned whether the base is monoprotic or polyprotic. Hence assuming it to…

Q: If a buffer solution is 0.560 M in a weak acid (Ka=5.3×10−6) and 0.120 M in its conjugate base, what…

A:

Q: If a buffer solution is 0.410 M in a weak acid (K, = 5.9 x 10-6) and 0.210 M in its conjugate base,…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5  pKa = -log Ka = - log ( 9.0 x 10-5)  pKa = 4.046 [Acid] = 0.200 M  [Conjugate base]…

Q: The pH of a (1.7300x10^-1) molar solution of an aqueous weak acid (HA) is (1.99x10^0). The Ka for…

A: PHis  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: A 0.050 M solution of a weak acid HA has a pH of 4.12 at equilibrium. What is the Ka of the acid?

A:

Q: Determine the K, of a weak base if a 0.28 M solution of the base has a pH of 10.14 at 25°C. K x 10

A: Given: Concentration of weak base (Assuming B) = 0.28 M And the pH of the solution = 10.14

Q: A weak base is dissolved in water with a concentration of 0.200 mol/L. The Kb value of the base is…

A: Given :- initial concentration of base = 0.200 mol/L                Kb of base = 9.75 × 10-4  To…

Q: what is the pH?

A: Given :-  Concentration of weak base = 0.120 M  Concentration of conjugate acid = 0.590 M  Kb = 5.9…

Q: what is the pH

A:

Q: If a buffer solution is 0.140 M in a weak base (Kb= 1.8*10^-5) and 0.590 M in its conjugate acid,…

A:

Q: If a buffer solution is 0.240 M in a weak acid (Ka = 8.1 × 10-5) and 0.430 M in its conjugate base,…

A: Given,Concentration of salt is given as a 0.430 MConcentration of acid is given as a 0.240 M

Q: A Moving to the next question prevents changes to this answer. estion 2 What is the pH of the…

A:

Q: If a buffer solution is 0.250 M in a weak acid (?a=2.3×10^−5) and 0.440 M in its conjugate base,…

A:

Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO¯ and 0.41 M in HIO? The K, for HIO is 2.3…

A: Given: Volume of solution = 80.0 mL Molarity of IO- = 0.27 M Molarity of HIO = 0.41 M Ka of HIO =…

Q: Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5. RICE Table is…

A: RICE table is the initial, change and equilibrium concentration of chemical species taking part in a…

Q: 6. If a buffer solution is 0.290 M in a weak acid (Ka = 3.3x10-) and 0.510 M in its conjugate base,…

A:

Q: A 0.0310 M  solution of an organic acid has an [H+] of 1.55×10-3 M . Using the values above,…

A: Given: A 0.0310 M  solution of an organic acid has an [H+] of 1.55×10-3 M .

Q: A certain weak base has a Kp of 8.60 × 10-'. What concentration of this base will produce a pH of…

A: Kb = 8.40x10-7 pH= 10.37 Concentration of base=?

Q: If a buffer solution is 0.180 M in a weak base (Kb=7.5×10−5) and 0.400 M in its conjugate acid, what…

A:

Q: If the K of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH =

A:

Q: If a buffer solution is 0.210 M0.210 M in a weak acid (?a=5.0×10−5)Ka=5.0×10−5) and 0.490 M0.490 M…

A:

Q: Sulfurous acid, H,SO,, is a weak acid capable of producing two ions. A) What is the pH of a 0.45 M…

A: Answer: Sulfurous acid is a weak acid which will give 2 hydrogen ions on adding in water and an…

Q: If the K of a weak base is 5.6 × 10-6, what is the pH of a 0.40 M solution of this base? pH

A: Given:  Kb = 5.6×10-6 Concentration = 0.40 M Since, the value of Kb and concentration of base is…

Q: If a buffer solution is 0.200 M in a weak base (K = 1.9 x 10-5) and 0.420 M in its conjugate acid,…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: If a buffer solution is 0.200 M in a weak acid (K = 7.1 × 10-) and 0.500 M in its conjugate base,…

A: We have given that  Weak acid = [HA] = 0.2 M Ka = 7.1×10-5  Conjugate base of acid = [A-] = 0.5 M

Q: If a buffer solution is 0.270 M in a weak acid (Ka = 7.5 x 10) and 0.570 M in its conjugate base,…

A:

Q: If a buffer solution is 0.300 M in a weak base (K₁ = 8.7 x 10-5) and 0.400 M in its conjugate acid,…

A:

Q: If a buffer solution is 0.270 M in a weak base (K, = 1.3 × 10-) and 0.450 M in its conjugate acid,…

A: We have 0.27 M weak base , and 0.45 M of conjugate acid . We have to calculate the pH of this buffer…

Q: A 0.0490 M  solution of an organic acid has an [H+] of 9.00×10-4 M . Using the values above,…

A:

Q: If a buffer solution is 0.240 M in a weak acid (Ka = 3.8 x 10-5) and 0.530 M in its conjugate base,…

A: Introduction Henderson - Hasselbalch equation gets used to calculate the pH for any buffer solution…

Q: If a buffer solution is 0.260 M in a weak acid (K, = 5.3 × 10-5) and 0.470 M in its conjugate base,…

A: This question is based on the prior knowledge of the Handerson Hasselbach equation which determines…

Q: If a buffer solution is 0.260 M in a weak acid (Ka=2.4 •10^-5) and 0.560M in its conjugate base,…

A: Given : Concentration of weak acid = 0.260 M Concentration of its conjugate base salt = 0.560 M And…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.