What is the hydroxide ion concentration [OH-] in a solution that has pH = 3? Assume the solution at 25° C. O 1.0 x 10-14 M O 1.0 x 103 M O 3.0 M O 1.0 x 10-11 M O 1.0 x 103 M

Q: What is the concentration of H3O+ in a solution which has a concentration of OH- equal to 8.9 x…

A: Since for any solution at room temperature  [H+] X [OH-] = Kw = 10-14  where [H+] = concentration of…

Q: If you have 0.1 x 6x 10^23 hydrogen ions in 1L of solution, what is the pH? O A. 7 В.3 O C. 5 O D.…

A: The correct answer is given below

Q: If [OH" ] = 5.2 x 10-4 M, what is the pH ? pH РОН [H* ] [OH ] ? 5.2 x 10-4 M O -3.3 O 10.7 O -10.7 O…

A: given, [OH-] = 5.2 ×10-4 M

Q: If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of…

A: To calculate the pH of a 1.8 mol/L solution of hydrazine.  Given: Kb for hydrazine, N2H4(aq) = 1.7 x…

Q: What is the pH of a 0.200 M solution of HNO3? A 0.70 B 1.31 c) 6.18 (D) 8.53

A: Given, the concentration of HNO3 =0.200 Mwe are asked to calculate the pH of solution of HNO3

Q: A solution of HNO3 has a pOH = 9.45. Calculate the concentration of H3O+ ions in the solution.

A: Solution - According to the question - Given value -  pOH = 9.45 pH and pOH are related as, pH + pOH…

Q: What is the pH of a 0.25 M solution of NH3? Kb = 1.8x105 O 2.67 O 11.33 O 9.07 O 4.93

A: Given valuues from  the question, Salt concentration = c= 0.25 M Kb =1.8×10--5 then,

Q: What is the pH of 4.3 x 10-4 M NaOH (aq)? O 17.4 10.6 О 3.4 O -3.4 O 24.6

A:

Q: What is the approximate pH of a 0.5 M solution of NaOH? A O to 1 3 to 4 C 7 to 8 13 to 14

A:

Q: Calculate the pH of a 2.4 x 105 M HBr solution at 25 °C. O 2.45 O 11.69 O 4.62 O 9.38

A:

Q: What is the pH of .03 M NH4Br (aq)? O 3.13 O 9.25 O 10.87 O 1.52 O 5.38

A:

Q: What is the pH of a solution that has [H*] of 1.00 X 10-4? O-4 O 14 4 01

A:

Q: What is the pH for a 0.05M solution of hydrochloric acid (HCI)? O -0.3 O 6.95 0.05 1.3

A: HCl is a strong monobasic protonic acid.

Q: Place the following in order of increasing acid strength. HlO < H1O 2 < HlO 3 < HlO 4;

A: Place the following in order of increasing acid strength ---

Q: What is the pH of a 1.40*10^ -2 mol/L Ca(OH)2 solution? (NOTE: To determine the actual hydroxide…

A: Given : Concentration of Ca(OH)2 = 1.40 X 10-2 mol/L

Q: Calculate [H3O+][H3O+] given [OH−][OH−] in each aqueous solution. [OH−] = 4.2×10−12 M [OH−] =…

A:

Q: Calculate the hydrogen Ion concentration in moles per liter 1) pOH: 4.10 2) pOH: 6.56 3)pOH:…

A:

Q: What is the hydrogen lon concentration of an aqueous solution with a pH of 8.777 O a. 5.2 M O b.…

A: Since we know that pH = -log[H+]  Using the above formula we will calculate the concentration of H+…

Q: What is the pH of a solution with [H*] = 1.0 x 104 M? 0 7 O -4 O 4 O 10

A: The pH of the solution is defined as negative logarithm of the molar concentration of H+ ions.…

Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93

A:

Q: What is the pH of 3.1 x 105M HBr solution? O 4.09 O 4.51 O 8.1 O -4.09

A:

Q: The pH of 0.20 M HNO3 is O a. 0.63 O b. 1.58 O C. 0.70 O d. 0.20

A: pH  =  - log [H+ ]  Strong acids undergo complete ionisation in solution.  Thus, [H+] =…

Q: What is the hydroxide ion concentration of a solution with pOH =1.5?

A:

Q: What is the pH of 5.35 x 103 M H2CO3 (aq)? O 4.3 O 8.6 O 2.3 O 4.9 O 9.1

A: Concentration of H2CO3 = 5.35 × 10-3 M  pH of the H2CO3 = ?

Q: What is the pH of 7.8 x 105 M HNO3 (aq)? O 18.1 O 9.9 O 9.5 O 3.7 O 4.1

A:

Q: Suppose .0274 g of HCIO4 is dissolved in 425 mL of aqueous solution. What is the pH? O 4.19 O 1.19 O…

A:

Q: What is the pH of 8.1 x 105 M HCIO4 solution? Is it acidic, basic or neutral? O 4.09; acidic O 4.09;…

A: • The values provided in the question are:-     i) Concentration of HClO4 solution, [HClO4] = 8.1 ×…

Q: %. What is the pH of 0.0015 M solution of nitric acid? a. 1.41 c. 5.65 b. 2.82 d. IL.18

A: To calculate the pH of 0.0015 M solution of nitric acid.

Q: What is the pH of a 9.27*105 M solution of H3O? O 4.03 O 9.97 O 12.81 O 2.98

A: (10) Kool aid a powdered substance when added with water or solvent, will give a flavored sugary…

Q: What is the pH of a 0.20 M HCI solution? O 12.39 O 0.70 O 13.30 O 1.61

A:

Q: What is the hydroxide ion concentration, [OH-], for a solution having a pH of 9.60? OA 2.5 x 10-10 M…

A:

Q: Calculate [OH ]in an aqueous solution with a pH of 4.33 at 25°C. 6.3 x 10 6 O 3.8 x 10-5 O 2.1 x 10…

A: [19.]  pH = 4.33 (given)  [H+] = 10-pH  [H+] = 10-4.33  [H+] = 4.677 × 10-5 M Hence, [OH-] = 10-14 /…

Q: What is the pH of a 3.00 x 10−8 M solution of HClO4? 6.48 7.00 6.89 7.52 7.15

A: Applying formula  pH = - log[H+] = -log[H3O+]  Equation  HClO4(aq) ———&gt;  H+(aq)  +  ClO4-(aq)

Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: Which is the strongest acid of the following? A)HClO3 B)HClO2 C)HBrO D)HIO

A: In case of oxyacids, increase in oxidation number of a particular halogen atom increases the acidic…

Q: If the pH is 4, what is the pOH? O 4 O 10 O -10 0 4

A:

Q: What is the pH of an aqueous solution of HNO3 with a concentration of 3.33 x 10-3 M? О А. 5.5 о в.…

A: Given the aqueous solution of HNO3 with a concentration of 3.33×10-3we are asked to the pH of…

Q: Calculate the percent ionization in a 0.040 M NH3 solution, given that the pH of the solution is…

A: The concentration of the NH3 solution is = 0.040 M The pH of the solution is = 11.50 The percent…

Q: What is  the pH of an (aq) solution, [OH-] = 4.6 × 10-10 M.

A: pH is equal to negative logarithm of hydrogen ions

Q: Calculate the pH of a 0.125 M HNO3 solution.

A: Working formula pH = -log[H+]

Q: What is the percent ionization of an 3.5 M HF solution? (Ka=6.6 x 104) O 1.4 % O 0.22 % O2.4 % O 1.7…

A:

Q: What is the pH of a 0.20 M NaBrO solution? Ką for HBrO = 2.8 × 10-9. O2.78 O 3.45 O 11.39 O 8.76 O…

A:

Q: What is the pH of a 8.82 x 10-2 M solution of NaOH? O 12.9 O 10.9 O 6.91 09.90 O 1.05

A:

Q: What is the pH of a 0.015 M aqueous solution of barium hydroxide? A) 12.18 B) 12.35 C) 1.82 D)…

A:

Q: Determine the pH of 0.25M CH3COONA solution. Kg of CH3COOH = 1.8×105 Select one: 10.08 O 9.08 O 4.90…

A: Sodium acetate is a salt of a weak acid, acetic acid, and strong base, sodium hydroxide. The salt of…

Q: What is the concentration, in moles/liter, of the hydrogen ion, if pH of a solution is 7? O 1 x 10-7…

A: pH = -log(H+) So, H+ = 10-pH

Q: What is the pH of a 0.042 M HNO3 solution?

A: HNO3 is a strong acid and ionizes completely to give H+ ion. Using this we will calculate pH.

Q: What is the pH of 1.75 M NH3 (aq)? O 9.50 O 4.50 O 4.74 O 2.25 Ο 11.75

A: Solution :

Q: Calculate the pH of a 3.5 x 10-3 M HNO3 solutio O 2.46 O 3.46 O 0.54

A: The acidity of the solution is measured by the pH scale. pH scale ranges from value 1 to 14. The…

Q: Which of the following would you expect to be the strongest acid? HIO2 HBrO2 HClO2 HClO HIO

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.