7. The [OH-] of a solution is 1 x 10-2 M. Which of the following is correct? (A) The solution is acidic with an [OH] of 1 x 10-12 (B) The solution is basic with a pH of 12 (C) The solution is basic with a pOH of 12 (D) The solution is acidic with a pOH of 2

Q: is the pH of a solution with a pOH of 1.36? s the pOH of a solution with a [OH-] of 2.97 X

A: pH +pOH= 14 pOH = -log[OH-]

Q: 6) If the hydroxide ion concentration of a solution is 1.0 x 10° M Is it an acidic or basic…

A:

Q: The pOH of an aqueous solution of 0.552 M ammonia is .

A: pOH is defined as negative logarithm of hydroxyl ions.

Q: What is the pH of a 0.0810 M solution of HONH;CI (Kb of HONH2 is 1.1 x 108)?

A: Given,                HONH3Cl -----> HONH3+ + Cl-  Hydrolysis of the weak conjugate acid, HONH3+…

Q: What is the pH of a 0.0500 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: HONH3Cl is a salt and in solution it gets dissociated as HONH3Cl → HONH3+ + Cl- The hydrolysis…

Q: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: What is the pH of a 0.0250 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH can be calculated as follows

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: An aqueous solution with a pH of 7 has a pOH of 4 O 10 14

A: Acids are the chemical compounds that donate proton, H+ in the solution, while base is the chemical…

Q: Calculate [OH¯] for a solution where [H,O*] = 0.00379 M. %3D [OH¯] = M

A: For an aqueous solution, we know that the production of the concentration of the hydrogen ions and…

Q: How would the pH of a 0.175 M solution of NaC4H,O2 compare with that of a 0.175 M solution of…

A: The salt gets hydrolyzed when dissolved in water. Both salt have the same acid and similar strong…

Q: Calculate the PH and pOH for eacho the solutions with the fo11owing hydngo 1on or hydrxide ion…

A:

Q: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca1OH22?

A: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca(OH)2?

Q: Which is the strongest acid of the following? HIO HBRO НOAt HCIO HCIO2

A: Order of acidic strength in the oxoacids of halogens: It depends upon the ability to donate H+ ion.…

Q: Arrange the following in order of INCREASING acidity. I. II. III. IV. ... ÇI CI HO HO HO HO

A: Given question of mainly phenol group.    We have difine a increasing acidic order.    Attached a…

Q: A solution with a pOH of 5.55 has an [OH–] of __________

A: We know,                            pOH = - log[OH-]                    Or, log[OH-] = - pOH…

Q: Calculate the hydrogen ion (H") concentraion of a solution with pH of 1.06

A: Given that, pH= 1.06

Q: A 4.9 × 10−3−mol sample of HY is dissolved in enough H2O to form 0.090 L of solution. If the pH of…

A: given, number of moles of HY = 4.9 × 10−3 Volume of solution = 0.090 L the pH of the solution = 2.55

Q: The pH of an aqueous acid solution is 6.15 at 25°C. Calculate the K, for the acid. The initial acid…

A: Given :-  initial concentration of acid = 0.012/M  pH of solution = 6.15  To calculate :-  Ka of…

Q: 2. The pH of a lime is 1.90. What is the [H3O*]?

A: pH is negative log of Proton concentration.

Q: A 0.250-mol sample of HX is dissolved in enough H₂O to form 655 mL of solution. If the pH of the…

A: Ka of HX can be calculated as follows,

Q: the pH of an acid solution is 3.59. If the concentration of the acid in the solution is 0.200 mol/L,…

A: Given Concentration of the acid=0.2 mol/LpH of the acid solution=3.59Ka of thel acid=??

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (a) 0.10 M…

A:

Q: What is the pH of a 0.580 M solution of C3H,NHB (Kb of CsH;N is 1.7 × 10-º)?

A: pH is the negative logarithm of concentration of hydrogen ion. pH of a solution can be calculated…

Q: What is the pH of a solution that is O.245 MH2S and 0.160 M sodium hydrogen sulfide (NaHS)? The Ka…

A: The reaction between Hydrogen sulfide and sodium hydroxide is

Q: What is the pH of a 0.0760 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: Given salt is a mixture of W.B + SA  HONH3Cl it undergo salt hydrolysis  It's  pH = 7 - 1/2(pkb +…

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

A:

Q: Calculate the pH of 2.5 M CH2ClCOOH(aq) given that its Ka = 0.0014.

A:

Q: Which of the following compounds are more acidic and WHY? Draw equations showing the dissociation…

A: An increase in the number of electronegative atoms will increase the acidity of the acid. If there…

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solution 0.035 M Na2S

A: 0.035 M Na2S hydrolyze in water to produce OH- ions. The ICE table is as follows:

Q: 2. The pH of a 0.100 M weak acid solution is 4.07. Calculate the K, value for the weak acid.

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: Given that the pH is 10.285 What is the: [H3O+] pOH [OH-] Is it an acid or base?

A: It is given that the pH of a solution is 10.285 and the [H3O+], the pOH and [OH-] needs to be…

Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: What is the pH of a solution that is 0.100 M in NaHCO3?

A: Given, 0.100 M in NaHCO3

Q: the pH of the solution containing 0.04 M H3PO4

A:

Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: C D B

A: Bronsted-Lowry Acid is any species that can donate a proton. When an acid and base react with each…

Q: The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is

A:

Q: Which of the following is the strongest acid: н, с. ОА Ов C OD A 'OH H, C FH В OH HC C OH F ж Н D…

A:

Q: is acidic or cor [H*]

A:

Q: What is the pH of a 0.380 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: What is the pH of a 0.0380 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH = 3.73

Q: Calculate the pH of a 2.00 M NH,CN solution,

A: NH4CN is a salt made up of weak acid, HCN (Ka = 6.2×10-10) and a weak base NH4OH (Kb = 1.8×10-5).

Q: The Kb of hydrazine is 9.1 x 10-7. If 3.12 x 10-3 mol of hydrazine is added to water to make up…

A: Hydrazine (N2H4) is a weak base Concentration of hydrazine is calculated as follows,

Q: The pH for a solution with an [OH] of 1.0 x 10^-6 is?

A: We have Concentration of OH- as 10-6 , we have to predict the pH of Solution.

Q: What substance(s) have a pH most similar to that of water (pH 7)?

A: Salt of strong acid and strong base have a pH similar to that of water i.e. pH = 7.

Q: What concentration of KNO2 must be added, at 25 degrees Celsius, to 0.50 M HNO2 to result in a…

A: The solution mixture is a buffer solution of weak acid HNO2 and conjugate base NO2- ( as KNO2…

Q: The pH of an aqueous solution of 0.114 M ammonium iodide, NH4I (aq), is This solution is acidic…

A:

Q: What is the pH of a 0.975 M solution of acetic acid, HC2H3O2?

A:

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.