5. What is the pH when [H+] = 3.9 x 10-4? 6. What is the [H*]when pH = 9.86?

Q: pH:    [H+]: 10-4  pOH:    [OH-]:

A: Calculation given as follows

Q: Determine the OH-, pH, and pOH of a solution with a H+ of 5.0 x 10-9 M at 25 °C. [OH"] = M pH РОН %3…

A: The acidity and alkalinity of a solution depends upon the concentration of hydronium ion and…

Q: the pH of a solution with [Ha0*]-1 × 109 M?

A:

Q: What is the pH of a neutral solution at 10°C, where Ku equals 3.6 × 10-18? pH =

A: Given : Kw at 10 oC = 3.6 X 10-15  Since in neutral solution, the equilibrium reaction taking place…

Q: 8. a. What is the pH if the [OH-] = 5.83*10-6? b. What is the pH if the [H] = 7.38*10-11? c. What is…

A: The pH of a solution depends upon the concentration of H+ ions present in it. More the concentration…

Q: 6. OH- concentration is 1.233x10(-7). What is the pH? 8.09 5.09 6.09 7.09

A: PH = -log [H+] POH= - log [OH-] Given [oH-]= 1.233×10-7

Q: What is the pH of a solution in which [H3O]+ is 2.2 x 10-12 M? Group of answer choices 2.34 4.54…

A: It is given that the concentration of H3O+ in the solution is 2.2×10-12 M

Q: What is the pH and pOH of a solution with [OH-] = 3.0 x 10-11M?  Is this solution acidic or basic?…

A: Applying formula PH= -log[H+]

Q: pH

A:

Q: What is the pH and pOH for water at 50°C? Kw (50°C)=5.48×10^-14

A: Given :

Q: What is the pH of a 2.4 M solution of H2CO3? (Ka of H2CO3 = 4.3 x 10-7, Ka of HCO3- = 7x 10-11)

A:

Q: What is the pH of a solution at 25 C if the [OH-] = 5.0 x 10-3 M?

A: pH measures the acidity of a solution. If pH is greater than 7 then solution is basic. If pH is less…

Q: What is the pH of a solution at 100o C if [OH-] = 6.3 x 10-12

A: pH = -log[H+]  [H+].[OH-] = Kw

Q: In neutral solutions: O a. [H+] = [OH-] (pH=7) b. [OH-] = 10.5 mol/L O C. [H+] = 10.5 mol/L d. [H+]…

A:

Q: 1) Complete the entries in the following table: .fAol od: [H*][OH] pH pOH Acid, base or neutral?…

A: The expressions useful to complete this table: [H+][OH-]=10-14 pH=-log [H+] pH+ pOH =14

Q: Ka for ammonium, its conjugate acid. (NH4+) = 5.68 x 10^-10 Using the answer above, what is the pH…

A: Given: Ka = 5.68 x 10-10 Concentration of NH4Cl = 0.140 M

Q: Calculate the pH of 0.075 MNAOH. (a) 10.40(b) 11.12(c) 11.46(d) 12.88(e) 13.26 fhudrochloric acid is…

A:

Q: 49) Which of the following is a strong base? A) Sr(OH), B) Fe(OH), C) HCI D) H2 E) H,0

A: Strong base:

Q: (Q19) What is the pH of a solution that is 0.768 in hydrosulfuric acid (H2S)? Ka1 = 8.9 x 10-8 and…

A:

Q: What would be the concentration of OH- of an acetic acid solution that has a pH of 3.88? O a. 1.3 ×…

A:

Q: Find the PH and tell if it’s acid or base [H+]=1.0 X 10^-1 M

A:

Q: (Q19) What is the pH of a solution that is 0.720 in hydrosulfuric acid (H2S)? Ka1 = 8.9 x 10-8 and…

A: PH of H2S can be calculated as follows

Q: find [H3O+] in M ph=2.00

A: Given,  The pH of the solution is 2.00 The [H3O+] is:

Q: In the reaction H2CO3 + H20 - HCO3 + H30*, the Brønsted acids are H20 and Hҙо* H30* and H2CO3 О нсоз…

A: Here from the given acid - base reaction ,we have to predict the Bronsted acids.

Q: Be sure to answer all parts. Determine the pH of the following solutions at 25°C. (a) [H,0*]=1.41 x…

A: The value of pH of the solution is determined from the presence of the concentration of the…

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: What is the pH if: and What is the pOH if:

A:

Q: The [H+] of a solution whose pOH = 11.13 is 1.35 x 10-3M. is this true or false

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: What is the pH of 0.015 M CH2FCOOH? CH2FCOOH + H2O + H3O* + CH2FCOO" Ka = 2.6 x 10-3

A: The ionisation reaction of the acid is written as  CH2FCOOH (aq) + H2I (l) -------> H3O+ (aq) +…

Q: 15. What is the molarity of an aqueous NH solution that has a pH of 11.17? Kb= 1.8 x 10-5.

A:

Q: find [OH-] and [H3O+] if the pH= 2.75

A:

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: Convert the following pH or pOH values to [H*] or [OH] concentration Example: pH = 7.0, [H*] = 1.0 x…

A: Note : As per our company guidelines we are supposed to answer only first 3 sub-parts. Kindly repost…

Q: : Find the Kw of pure water at 50.0°C, if the pH is 6.630? 2: Find the pOH in an aqueous solution…

A:

Q: Find the a0 and a1 values ​​of hypochlorous acid in a solution with a pH of 7.0. (Ka = 3x10^-8 for…

A:

Q: Fill in the rest: (Use only the exponent for H and OH) pH:  H+:  pOH:  OH-: 10-4

A: [OH-] = 10-4 (given )  pOH = - log [OH-]  pOH = - log (10-4)  pOH = 4  Since, we know that ; pH +…

Q: 1. What is the pH of a solution in which the [OH-] is 1.5 x 10-52

A: Given:                            [ OH- ] = 1.5 ×10-5 Asked for:                            pH =…

Q: Find the pH of a 0.247 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C. 11.32 2.68…

A:

Q: What is the pH of a 0.02M ammonia solution if its Kb value is 1.8*10^-5? H,O + NH, 2 OH- + NH,. 3.2…

A:

Q: What is the pH of a solution when [OH−] = 6.4 x 10-3?

A: Given :- [OH−] = 6.4 x 10-3 M  To calculate :- pH of solution

Q: Calculate the pH of a 0.24 M solution of weak base A-1 that has a Kb of 2.5 x 10-6.

A: Weak bases are does not dissociate completely into ions in the solution, equilibrium is formed…

Q: 3.) The same solution in Question 17 has [H+] = 3.2 x 10-10. What is the concentration of OH-?…

A:

Q: Kw = 0.114 x 10-14 at 0°C = 1.00 x 10-14 at 25°C Kw Kw = 2.42 x 10-14 at 37°C Kw = 9.61 x 10-14 at…

A:

Q: Fill in the rest: (Use only the exponent for H and OH) pH:  H+: 10-5 pOH:  OH-:

A: For the given solution the concentration of the hydrogen ion is = 10-5 For this solution, pH =? pOH…

Q: What is the pH of the resulting solution if 100.0 mL of 0.10 M NAOH is added to 50.0 mL of 0.84 M…

A: Lactic acid is a weak containing one acidic hydrogen. Dissociation of weak acid lactic acid takes…

Q: What is the pH of 0.45 M NaF?

A: Given : Concentration of NaF = 0.45M

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.

Q: 2. Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Find the concentration of H1 in a solution whose pH is 11.65.

A: The question is about to calculate the concentration of H+ in a solution whose pH is 11.65 -

Q: Analyze the given parameters before ticking the right answer * pOH = 3 [H+] = 4.2 x 10-3 [OH-] =…

A: Acid is a substance  having PH less than 7. Base is a substance  having PH  greater than 7. In case…

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.