13. What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?   Group of answer choices 3.0 2.52 -2.52 9.0 3.0 × 10-3     14. What is the pH of a solution with [OH-] = 2.0 × 10-10 M?   Group of answer choices 9.70 4.30 -4.30 -9.70 2.0 × 10-10

Q: A scientist dilutes 50.0 mL of a pH 5.85 solution of HCl to 1.00 L. What is the pH of the diluted…

A: Given data,pH=5.85Volume of HCl=50mL=0.050LDilution=1.0LKw=1.0×10-14

Q: Calculate the pH of 0.40 M NH3 (Kb=1.8×10−5) Calculate the concentration of NH3 present in 0.40 M…

A:

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: A solution is made from 0.51 M NH3 and 0.48 M NH4Cl. What is the pH if the Kb for NH3 is 1.8x10-5?…

A:

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 solution of pyridine that contains 4.15 x 10^-4 hydroxide ion. Group…

A: Given, [OH-] = 4.15×10-4 M pOH = -log[OH-] pOH = -log[4.15×10-4 ] pOH = 3.38

Q: Given the Kb of C6H5NH3+ is 3.98x10-10 : 1.) What is the [H3O+] concentration in a solution that is…

A: Given,  Given the Kb of C6H5NH2  is 3.98x10-10 : The [H3O+] concentration in a solution that is…

Q: Calculate the [H+] in a solution that has a pH of 12.01. 9.8 × 10-13 M 12.0 M 2.0 M 1.0 × 10-2 M…

A: Given    PH = 12.01          -log[H+] = 12.01            log[H+] =  -12.01           [H+]  =…

Q: The weak base, B O H, has a K b value of 3.9E-5. Calculate the pH of this solution if the…

A: Given: Kb of BOH = 3.9×10-5 Concentration of BOH = 0.706 M

Q: Morphine is a weak base with a Kb = 1.6 x 10-6. What is the pH of an 0.83 M solution of morphine?

A: Given data,Kb=1.6×10-6Molarity=0.83M

Q: Calculate the [H+] for (a) black coffee with a pH of 4.42 (Enter your answer as follows: 1.0E-2 for…

A: (a) pH can be written as - pH = - log [H+] [H+] = Antilog (- pH) [H+] = Antilog ( - 4.42) [H+] =…

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: Calculate the pH of a solution with a H3O+ concentration of 4.76 × 10-4 M.   3.32 10.68 5.45 4.76

A: Given, [H3O+] = 4.76 x 10-4 M

Q: The diprotic acid H2A has Ka1 = 4.2 x 10-7 and Ka2 = 4.7 x 10-11. Calculate the pH of a 0.080 M…

A:

Q: The pH of 750 mL (3 SF) of an aqueous solution containing only NaNO 2 is 8.42. If HNO 2 has a Ka of…

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: Normal human blood has a hydroxide ion concentration that ranges from 1.7 × 107 -7 M to 3.5 x 10 7…

A: Given: pH of blood = 7.67  And the normal range of hydroxide ion concentration in the human body is…

Q: An aqueous solution has a hydronium ion concentration of 2.0 x 10-10 M. What is the pH?   2.00…

A: Given that an aqueous solution has a hydronium ion concentration of 2.0 x 10-10 M. The pH of the…

Q: Determine both the H and the pH in a 0.0541 M solution of HNO3 at 25 °C? H= Type your answer here…

A: The concentration of HNO3 solution = 0.0541 M HNO3 → H+ + NO3− The concentration of H+, [H+] =…

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: Calculate the pH of a solution of 0.100 M H2SO3. Ka1 = 1.23 x10-2 Ka2= 6.6 x 10-8

A: First dissociation                                                                2nd…

Q: Determine the pH of 0.080 M NH4Cl (pKa = 9.3). Give your answer to two decimal places.

A: Note - Since you have asked multiple questions, we will solve the first question for you. If you…

Q: Calculate the pH of 0.200 M HNO3(aq). 1.609 -1.140 0.699 2.000 13.800

A:

Q: What is the pH of a 5.58×10-5 M solution of the strong acid HCl? HCl(aq) + H2O(ℓ) → Cl-(aq) +…

A: The pH of the two solution has to be determined. The formula to calculate the pH is,…

Q: Calculate the [H+] for: (a) black coffee with a pH of 4.88 (Enter your answer as follows: 1.0E-2…

A:

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: Find the pH of a solution 0.9 M in HNO2, and 1.0 in NaNO2. For HNO2 Ka= 4.0 x 10^-4 Report answer to…

A:

Q: What is the pH of a 0.0020 M HCl solution?   a. 11.30   b. 0.0020   c. 0.0040   d. 8.80   e.…

A:

Q: The venom of stinging ants contains formic acid, HCOOH, Ka = 1.8 × 10-4 at 25 oC. Calculate the pH…

A: •GIVEN:- Formic acid which is an weak acid.  Ka = 1.8 × 10-4 Concentration (C)=0.055 M   •As for…

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: . Calculate the pH of .01 M NaOH A. 12 B. 2 C. 14 D. 1   2. Calculate the pH of .01 M HCI  A. 2 B. 1…

A:

Q: What is the pH of a solution with a hydronium ion concentration of 3.9x10-7 Record to the tenth's…

A:

Q: If a 1.0 M acid solution has a pH of 1.58, what would be the pH of a 0.10 M solution of the same

A: We have to find pH of given solution

Q: If the [H3O+] is 4.95 x 10–12 M, what is the pH?

A: Given :-  [H3O+] =  4.95 x 10–12 M  To calculate :- pH of solution

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

A:

Q: What is the [OH-] for a solution with a pH of 1.68? a) 2.1 x 10-2 mol/L b) 2.09 x 10-2 mol/L c)…

A:

Q: alculate the pH of a solution of 0.100 M Na2SO3. Ka1 = 1.23 x10-2 ; Ka2= 6.6 x 10-8 A. 4.55 B. None…

A: Sodium Sulphite (Na2SO3) is regarded as the fully deprotonated form (SO32-) of diprotic acid H2SO3.…

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: V. Milk of magnesia has a pH of 10.2. What is the [OH] of milk of magnesia? pH= 162 =) plO H)= 3.8…

A:

Q: Calculate the pH of a 0.55 M solution of ammonia given that Kb= 1.8 x 10-5 for ammonia. b)What is…

A: a) The decomposition of NH3 will take place as follows:…

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: What is the pH of a solution with 10.0mL 0.1M NH3 and 0.15mL 1.0M HCl ? Kb = 1.8x10^-5

A:

Q: the pH of a solution with an [OH-] =  8.95x10-11 M

A:

Q: What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion? A)…

A: Given : Hydronium ion concentration = [H3O+ ] = 3.98 X 10-9 M

Q: Determine the pH of a 0.625 M NH3 solution. The Kb of NH3 is 1.85 × 10-5.

A: Given,  The pH of a 0.625 M NH3 solution is: The Kb of NH3 is 1.85 × 10-5.

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.