What is the pH of asolution that is 0.063 Min HA and also 0.023 Min NaA? (Ko = 4.1 x 10-6)%3DO 4.95O 5.11O 6.23O 5.46O 7.15

given, concentration of HA = 0.063M concentration of NaA= 0.023M Ka = 4.1×10-6

Answered: What is the pH of a solution that is…

What is the pH of a solution that is 0.063 M in HA and also 0.023 M in NaA? (Ka = 4.1 x 10-6) %3D O 4.95 O 5.11 O 6.23 O 5.46 O 7.15

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter15: Solubility And Complex Lon Equilibria

Section: Chapter Questions

Problem 105CP: What is the maximum possible concentration of Ni2+ ion in water at 25C that is saturated with 0.10 M...

See similar textbooks

Related questions

Q: What is the pH of a solution with [H3O+]=2.42 x 10-4?

A: pH of any solution is given by pH = -log[H3O+] where [H3O+]= concentration of H3O+ ions

Q: A solution is prepared by dissolving 4.50 g of solid NaOH in 1.00 L o 0.100 M HNO₂(aq) (Ka =…

A: The pH of the solution can be calculated as follows

Q: What is [H] in a 0.430 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 × 10 5)? %3D

Q: 1. The oxalate ion concentration, C;0. of 0.20 M H;C0 is adjusted to a value of 3.00 x 10 M. What is…

A: As per the guideline, since you have asked multiple questions, we have solved the first question for…

Q: What is the pH of a 0.35 M solution of hydrofluoric acid with a Ka of 6.6 x 10-4? О 3.23 O 5.47 O…

A: Given: Concentration of HF = 0.35 M Ka of HF = 6.6x10-4

Q: Calculate the pH of a 0.6 M solution of Na,S. For H2S: Ka1 = 9.1x10 Ka2 = 1.2x10 15 a. 7.18 b. 14.35…

A: NOTE: the answer is not matching with the exact solution out of the options given. so, I have…

Q: The mg/L concentrations of 2.50x104 M solutions of HNO, (F.wt 63 g/mol) equal. 15.57 15.75 17.5 15.5

Q: Calculate the pH of a 0.053 M NaF solution. (Ka for HF = 7.1 x 10−4.)

A: NaF is a salt of strong base (NaOH) and weak acid (HF)

Q: What is the percent ionization at 25 °C for a 0.00675 M solution of codeine (CH2, NO)? O 18.7% O…

Q: As2. .. What is the minimum pH needed to prepare 1% sodium phenobarbital in water? Intrinsic…

A: We have to prepare 1% sodium phenobarbital in water. Solubility = 0.004M MW = 232.2g/mol pKa = 7.41

Q: 8. What are the [H3O+] and [OH–] of Diet Coke that has a pH of 3.17?

Q: What is the pH of a 0.01 M CH3COOH solution? (Ka= 1.74 x 10-5)

A: Given that Ka of Ch3COOH is 1.74× 10^-5 Concentration of Ch3COOH is 0.01M

Q: What is the pH of a solution that is 0.0032 M in HA and also 0.087 M in NaA? (Ka = 4.1 × 10-6) 6.56…

Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 x 10-5) %3D O 4.94 O 2.09 11.05 O 12.03 8.02

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the…

Q: How many grams of lithium formate (LiCHO2) need to be dissolved in 184 mL of a 0.664 M formic acid…

A: Given: Concentration of HCHO2 i.e. the weak acid = 0.664 M Volume of solution = 184 mL = 0.184 L…

Q: 5. A solution of nitrous acid has a pH of 2.45. The [H'] in mol/L and pOH must be respectively a.…

A: Given:…

Q: Phenylammonium is a weak base with a K,= 4.3 x 1o 10. What is the pH of a solution with an ammonia…

A: NOTE : In question, instead of phenylammonium, ammonia is mentioned by mistake. Hence I'm assuming…

Q: What is the pH of 1.10 M CrCl3 (K = 1.00x10-4)? %3D

A: Given, Concentration of CrCl3 (C) = 1.10 M Ka = 1.00 × 10-4 pH of the solution = ? Note: pKw = 14…

Q: Which of the following is strongest acid HA (pka = 1) HB (pka = 2) HD (pa = 3) НЕ (pка — 4)

A: Pka of acid is given by the negative logarithm of Ka i.e pKa = -log Ka where Ka is the acid…

Q: Calculate the concentrations of SO32−, H3O+, and OH− in a 0.510 M solution of H2SO3 (Ka1=1.6×10−2…

A: Given: The concentration of H2SO3 (sulfurous acid) is 0.510 M The value of Ka1 ( first acid…

Q: Calculate the pH of 0.0154 M NaN3 Given: Ka of HN3 = 1.9 x 10-5

A: The pH of a solution is used to determine the acidity or basicity of a solution. The pH is…

Q: What are the [H,O*| and [OH] of Diet Coke that has a pH of 3.17? ()

Q: What is the pOH of 0.003M acetic acid solution (Ka = 1.8 * 10 ^ - 5) O 11.4 O 10.4 O 3.3 O 4.6…

A: pH is defined as negative logarithm of hydrogen ion concentration.

Q: What is the pH of a 0.36 M solution of HNO2 (Ka = 4.5 x 10-4)?

Q: What is the pOH of a solution with [H+] = 3.37 x 10-5 ?

A: given - [H+] = 3.37 x 10-5 pOH = ?

Q: What is the pH of a solution that is 0.063 M in HA and also 0.023 Min NaA? (Ka = 4.1 × 10- O. 5.46…

A: Given: The concentration of HA is 0.063 M The concentration of NaA is 0.023 M The Ka value is 4.1 x…

Q: Calculate the Ka of a 0.390 M acid solution with [H3O+]= 4.52 x 10-5M

Q: A 0.030 M aqueous solution of a sodium salt (NaA) has a pH of 8.23. What is the value of K, for the…

A: The correct answer is given below

Q: 3. Calculate the pH of a solution containing 0.10 M H3BO3 and 0.18 M NaH2BO3 Ka = 5.81 X 10 10

Q: MCQ 9: Oxides of group IV behave : A. acid B. base C. amphoteric D. alkalis

A: When elements of group IV react with oxygen, they give different oxides , which may be acidic ,…

Q: 24) What is the pH of a 0.570 M solution of aniline? Kb = 7.4 x 10-10 A) 2.6 В) 4.7 C) 11.4 D) 9.3…

A: The given aniline is a weak base and has Kb = 7.4 x10-10 . The equilibrium reaction for the aqueous…

Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?

Q: What are the concentrations of H3O+ and OH− in oranges that have a pH of 3.92?

A: pH is the potential of the hydrogen. It basically defines how acidic or basic the respective…

Q: What is the pH of a solution that is 0.03M in picric acid and 0.1M in sodium picrate. pka=0.38 O a.…

A: The solution is mixed by adding picric acid to sodium picrate. Sodium picrate is made by adding…

Q: What is the pH of a solution that is 0.048 M in HA and also 0.042 M in NaA? (Ka = 4.1 x 10-6) 6.82…

A: Given, Ka for NaA = 4.1 x 10-6 PH = ?

Q: If [H3O*] = 3.8 x 10-3 M, what is the pOH of the solution? %3D O 2.42 O 2.13 O 2.77 11.58

A: The given data contains, H3O+=3.8×10-3M.

Q: What is the pH of a solution with a fluoride concentration of 0.11 M ? The Kb for F– is 1.47×10-11 .

A: The reaction is as follows, The ICE table for above reaction is shown below,

Q: What is the pH of a 0.20 M NaBrO2 solution? Ka for HBRO2 =1.2 x 10 O 11.39 O 3.45 O 9.11 O 8.76 O…

Q: Find the pH of a 0.381 M aqueous solution of hypobromous acid (HOBr), for which Ka = 2.1 * 10-⁹.…

Q: What is the pH of a 0.1055 M CH3COOH solution (K, = 1.75 x 10-5)? %3D

A: Answer: ICE table for the dissociation of weak monoprotic acid is shown below:

Q: Calculate the pH of a 0.20 M solution of NaC2H302. HC2H3O2 has a Ka-1.8 O a. 8.56 O b. 7.00 Oc. 9.02…

A: The question is based on the concept of salt hydrolysis. We have to calculate pH of the Sodium…

Q: 13.2) What is the pH of a 0.85 M solution of sodium hydrogen sulfite, NaHSO3 (Ka=6.0 x 10^-8)?

A: Given: Initial concentration of NaHSO3=0.85 M Ka for NaHSO3 = 6 x10-8 We know that, pH = -…

Q: 11. What is the pH of 0.05 M NaNO2 solution? [Ka of HNO2 = 4.0 x 10-4] * O 8.0 O 6.0 O 5.0 O 3.4 9.0

Q: Calculate the pH of 0.0154 M NaN3. (Ka of HN3 = 1.9 x 10-5)

A: NaN3 is a salt of weak acid (HN3) and strong base (NaOH). We know, the pH of salt, which is formed…

Q: What is the pH of a solution that is 0.048 M in HA and also 0.042 M in NaA? (Ka = 4.1 × 10-6) %3D O…

Q: Find the pH of a 0.204 M KClO solution. (The Ka of hypochlorous acid, HClO is 2.9×10-8

A: Kclo is a salt of weak acid and strong base so use the formula of PH of salt. PH=10.4

Q: Calculate the pH of a 0.0325 M hypochlorous acid solution. [ K, = 3.0 x 10-8]. %3D O 9.49 O 4.51 O…

Q: What is the pH of a 2.5 M solution of the weak base ephedrine (Kb = 1.4 × 10-4)? O a. 13.30 b. 11.72…

Question

What is the pH of a
solution that is 0.063 M
in HA and also 0.023 M
in NaA? (Ko = 4.1 x 10-6)
%3D
O 4.95
O 5.11
O 6.23
O 5.46
O 7.15

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Would you expect an aqueous manganese (VII) oxide solution to have a pH greater or less than 7.0? Justify your answer.
What is the maximum possible concentration of Ni2+ ion in water at 25C that is saturated with 0.10 M H2S and maintained at pH 3.0 with HCl?
A hypothetical weak acid, HA, was combined with NaOH in the followingproportions: 0,20 mol HA, 0,08 mol NaOH. The mixture was diluted to a totalvolume of 1,0 L and the pH was found to be 4,80. a). What is the pKa of the acid?
What is the percent ionization of nitrous acid in a solution that is 0.230 M in nitrous acid (HNO2) and 0.270 M in potassium nitrite (KNO2)? The acid dissociation constant of nitrous acid is 4.50 x 10-4.
Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.
11.(a) 10.06 cm3 of the stock 0.100 mol dm–3 solution of NaOH was required to fully neutralise 49.5 mg of a diprotic acid (H2A). Write a balanced equation for this reaction and hence determine the molar mass (Mr) of the acid. (b) Determine the pH of 0.100 mol dm–3 NaOH at 298 K [pKw = 14.0].
How many grams of K2A (M. W. 166.22) should be added to 15.0 mL of 0.200 M HCIO4 to give a pH of 4.70 when the solution is diluted to 500 mL ? The acidity constants of H2A are 5.36 x 10-2 and 5.42 x 10-5,
A solution is made by dissolving 0.111 moles of N2H4 (Kb = 3.0 x 10-6 ) and 0.199 moles of N2H5Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?
5. A solution of H2SO4 is found to be 0.5172 N and 39.65 mL of it are equivalent to 21.74 mL of standard alkali solution. What is the N of the alkali and how many grams of sulfamic acid (HSO3.NH2) will 1.00 mL of it neutralize?
What is the pH when preparing a solution od 1 mol NaOH and 2 mol of solid NaH2PO4? The pKa's of phosphoric acid are: 2.1, 7.2, and 12.4.
How many grams of potassium lactate (C3H5O3K) need to be dissolved in 129 mL of a 1.71 M lactic acid (HC3H5O3, Ka = 1.4 × 10−4) solution, so that the pH of the solution is 4.22? Report your answer to THREE significant figures.
1) For an open system with PCO2=10−3.5 atm what fraction of the total carbonate is in the form of CO32− at pH 10.63? 2) Using paleolimnological methods it is possible to estimate past pH values of surface waters. If the estimate of pH is 5.787 , what is the corresponding PCO2? in atm.