What is the ph of 2.11M HC2H3O2 if ka=1.8x10-5? What is the ph of 3.50M HCN if ka=4.9x10-10 What is the ph of 1.50M HClO2 if ka=1.1x10-2

Q: 8. What is the PH of a solution with [H*]=1 x 10-³M ]3 2HCNO ]-3HF |-2 ]None of the others 9. What…

A: Hello. Since more than one question has been asked, the first question shall only be answered in…

Q: Calculate [H2Asc], [HAsc-], [Asc2-], and the pH of 0.050 Mascorbic acid H2C6H6O6, H2Asc. (Ka1=…

A: We have given that Molarity of ascorbic acid = 0.050 M  Ka1 = 1.0×10-5  Ka2 = 5 × 10-12

Q: What is the pH of an acetic acid solution (HC2H3O2) with concentration 0f 0.100 M. Ka=1.75 x 10-5 A.…

A: An ICE table is constructed to determine the equilibrium concentration of H3O+ as follows,

Q: What is the pH of a 0.0015 M solution of HBr?     5.65     You need the Ka value to answer this…

A: What is the pH of a 0.0015 M solution of HBr?

Q: Calculate the pH for an aqueous hydroiodic acid solution that contains 3.15 x 10^-3 hydronium ion.…

A: pH is the negative logarithm of Hydrogen ion (hydronium ion) concentration. It stands for power of…

Q: Arsenous acid, H3AsO3, pKa2 = 7.00. What is the pH of a solution made up to have [H3ASO4) = 1.00 M…

A: In this question, we have to find out the correct answer of given problem by the help of henderson…

Q: Which of the following aqueous solutions will have the highest pH? For NH3, Kb = 1.8 × 10–5; for…

A: Here we have to find out the respective ph of all the species

Q: Calculate the [H+] for (a) black coffee with a pH of 4.33 (Enter your answer as follows: 1.0E-2 for…

A: pH = -log [H+]

Q: Calculate the pH of a solution containing 0.0361 M benzoic acid (HC>H502) and 0.0263 M sodium…

A: The given mixture is a buffer solution mixture. So, this can be solved from the Henderson…

Q: What is the [H3O+] in a solution with a pH of 8.66? Group of answer choices 2.2 × 10-9 M 1.5 × 10-5…

A:

Q: What is pH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10…

A: 1.05 M NH3 and 0.98 M NH4NO3 The NH4NO3 dissociate as ; NH4NO3 =  NH4+  + NO3-  So the Concentration…

Q: Calculate the pH of a solution being 0.185 M in HNO2 (Ka=4.6x10^-4) and 0.085 M in HNO3. ( answer to…

A: PH = -log [H+] Where [H+]= concentration of H+ ion .

Q: a chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She dound…

A:

Q: Calculate the pH of 0.05 M Ba(OH)2 Group of answer choices 1.3 2.6 1.0 13

A:

Q: solution of this acid is found to have a pH of 2.607. Based on the table below, what most likely is…

A:

Q: What is the pH of 0.1000 M Na₂HPO4? (K₁2=6.2x10-8, K3=4.8x10-13) What is the pH of 0.1000 M Na3PO4?…

A: The solutions considered are 0.1000 M Na2HPO4 and 0.1000 M Na3PO4. The question requires to…

Q: Determine the pH of a 0.275 M KOH solution. Give your answer to 2 decimal places in regular…

A:

Q: What is the pH of a solution with [H3O+] =  1 x 10-9 M? Group of answer choices 1 x 10-5 9 5 -5

A:

Q: 13. What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?   Group of answer choices 3.0 2.52…

A: pH :-  The negative logarithm to the base 10 of hydronium ion concentration , [H3O+] expressed in…

Q: Calculate the pH of a 2.80×10-1 M aqueous solution of sodium acetate (NaCH3CO2). (For acetic acid,…

A:

Q: Determine the pH of each solution. 0.10M NH4Cl0.10M NH4Cl 0.10M NaC2H3O20.10M NaC2H3O2 0.10 M…

A: In this question, we have to find out the correct answer of given problem by the help of pH concept.…

Q: What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH? (The Ka value for benzoic acid is…

A: given :- concentration of benzoic acid = 0.40 M  Ka for benzoic acid = 6.3 × 10-5  To calculate :-…

Q: The pH of a 8.3×10-2-M solution of phthalic acid (H2C8H4O4) is measured to be 2.03. Use this…

A:

Q: The kw for water is 5.5 x 10-14 at 50oC.  What is the pH of a neutral aqueous solution at 50oC?…

A:

Q: 1a) Determine the pH of 0.035 M NaF (pKa = 3.1).   1b) Determine the pH of 0.055 M oxalic acid…

A: It's a multiple part question.   Given information, 1 (a) [NaF] = 0.035 M pKa = 3.1 1 (b) [oxalic…

Q: Determine the pH of a 1.30 M solution of CH3COOK. Ka(CH3COOH) = 1.8×10-5 Express your answer to

A: 1- First Calculate the OH- ion concentration :  CH3COO- + H2O <------> CH3COOH + OH-   The…

Q: The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10.  What is the pH…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: What is the concentration of an aqueous HI solution that has a pH of 2.26?     1.82 x 10-2 M…

A: Given that, pH = 2.26  Then, [HI] = ?

Q: All of the following statements about the pH scale are true EXCEPT Group of answer choices: Blood is…

A: Using the relation of pH and [H3O+] , concentration of hydronium ion, [H3O+] can be determined.

Q: What is the concentration of hydrogen ion in a solution with a pH of 5?     1×1051×105 M 1 times 10…

A:

Q: What is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? The Ka of propionic…

A: Sodium propionate is a salt of weak acid and strong base. Given, Ka of propionic acid = 1.3x10-5…

Q: A 1.0 × 10 -2  M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of? 12.30     12.00     2.0 ×…

A: Answer:- This question is answered by using the simp[le concept of calculation of pH of the solution…

Q: Calculate the pH of a 0.18 M solution of KNO2. (Ka (HNO2) = 4.5 x 10-4) Group of answer choices…

A: Given : Concentration of KNO2 = 0.18 M And Ka of HNO2 = 4.5 X 10-4  Since KNO2 is a completely…

Q: What is the hydroxide ion concentration of a NaOH solution that has a pH of 12.20? Choose from one…

A: Given :-we have to find the hydroxide ionconcentration of a NaOH solutionthat has a p H of 12.20.

Q: pproximate the final pH of a solution when 1.5 moles of a weak acid is added to water to a final…

A: Given : Moles of weak acid = 1.5 Volume = 1L Ka =  5.67x10^-8

Q: Which of the following has the lowest pH?   3.9x10-3 M HPO42- (Ka3=4.2x10-13)   0.00010 M H3BO3…

A:

Q: Acetic acid is a weak acid with Ka = 1.8 x 10 -5 and ionizes into HC2H3O2 -------H + + C2H3O2 - What…

A: pH is negative logarithm of hydrogen ions

Q: The pH of certain orange juice is 4.54.  The hydroxyl ion (OH-) concentration will be. a. 4.47 x…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pH of a solution with 10.2mL 0.10M CH3COOH and 0.15mL 1.0M HCl ? Ka = 1.8x10^-5

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50 Group of answer…

A:

Q: What is the pH of a 0.370 M aqueous solution of methylammonium chloride, CH3NH3Cl? The Kb of methyl…

A:

Q: the pH of a solution of 15 g NH4Cl and 15 g of NH3 in a 850mL solution? The Kb for NH3 is 1.8 x 10-5

A:

Q: Calculate the pH of a 0.29 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.6…

A: The question is based on pH calculation. we have been given a weak acid. we have to calculate its…

Q: Calculate the pH of a 0.53 M HONH2 solution. Give your answer to two decimal places Kb(HONH2) = 1.0…

A:

Q: The Kb of (CH3)3N is 6.4x10^-5. What is the pH of a 0.48 M solution of (CH3)3NH+?

A: Given: The Kb of (CH3)3N = 6.4 × 10-5 We have to calculate the pH of a 0.48 M solution of (CH3)3NH+.…

Q: What is the final pH of a 2.86 M solution of arsenic acid, H3AsO4, where Ka1 = 5.5 x 10^-3, Ka2 =…

A:

Q: HIO3 has a ka of  0.16. What is the pH of a 0.600 M HIO3 solution? (use successive approximations)

A: The strength of an acid depends on the extent of its dissociation in water. Strong acids dissociate…

Q: What is the pH of a 0.070 M aqueous solution of methylamine, CH3NH2? The Kb for methylamine is…

A:

Q: Trimethylamine, (CH3)3N, is a gas with a fishy, ammonia–like odor. An aqueous solution that is 0.29…

A: The ionisation reaction of (CH3)3N is  (CH3)3N (aq) + H2O (l)  ------> (CH3)3NH+ (aq) + OH-

Q: What is the pH of 0.1510 M selenious acid solution, H2SeO3? H2SeO3(aq) + H2O(l) → HSeO3−(aq) +…

A: As the second ionization constant Ka2 is very less than first ionization constant Ka1, the Ka2 can…

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.