What is the pH when the hydrogen ion concentration is 1 x 10° M? O a) -5 O b) 9 c) -9 O d) 5

Q: 11

A: Step-1: Calculate the H+ Value [H+] [OH-] = 1 x 10-14 H+ = [1 x 10-14]/ [OH-] H+ = [1 x 10-14]/ [1 x…

Q: the pH of the solution given that Kw=2.93×10^−15 at

A: The pH of the solution given that Kw =2.93×10−15 at this temperature

Q: Calculate the pH of a HNO3 solution with a hydrogen ion concentration of .83M A. 0.08 B. 0.15 C.…

A: Given, [HNO3] = 0.83M

Q: What is the pH when the hydrogen ion concentration is 1 x 10^-9 M? O a) 5 b) -9 O c) 9

A: Hydrogen ion concentration = 1 x 10-9 M  pH = - log [H+]

Q: The pH of a neutral solution at 25°C is O 7 14

A: The pH is the negative logarithm of hydronium ion concentration. It is used to determine the acidity…

Q: What is the pH of a 0.00450 M HNO3 solution? A) 2.35 B) 3.52 С) 4.50 D) 11.65

A: We know that, pH of the solution can be expressed as negative logarithm of hydronium ion…

Q: 7. Calculate the [H3O'] from the pH for each of the following. [H,O'] pH (H3O'] pH 10.90 5.30 3.70…

A: Using the formula pH = -log10[H3O+] we can solve this problem.

Q: What is the pH of a 0.0060 M KOH solution? A) 5.12 B) 2.22 C) 11.78 D) 8.88

A: The quantity capable of predicting solutions' acidic nature is named as pH. It can be related with…

Q: What is the pH of a 0.2 M HNO2 solution if percent ionization is 1.2%?

A: PH = - log(H+) Percentage of ionisation = 1.2 HNO2 are in 0.2M

Q: Calculate the pH of the follo 0.39 M NH4CI (рКp fo O a. 2.57 O b.4.83 с. 9.67 O d.4.33 O e. none of…

A: Given, pKb = 4.74  Concentration of Salt(C)= 0.39 M It is salt of weak base -strong acid type salt .…

Q: If the pOH of a solution is equal to 9.33, the pH of the solution is equal to 3.39. O True O False

A: Given  pOH of the solution = 9.33

Q: The pH of a solution is 2.55. What is the[H3O+] A 2.8x10-3M B 2.55M C 2.0x10-15M D 0.28M

A:

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 of a solution with a concentration of hydronium ions of 5.11×10 with a little arrow…

A:

Q: What is the pH of a solution that has an [H+]=0.0470 M ? 3.06 12.7 1.33 8.42

A: We have to calculate the pH of Solution.

Q: What is the concentration of 5% White Distilled Vinegar based on the pH value?  [H+] = ? M  given…

A: The given pH is 2.22. From the pH value, the concentration of H+ can be found from the equation,…

Q: What is the pH of a 3.21 ×10 -2 M solution of KOH?   1.49 9.97 12.5 6.97

A: Given, Concentration of the KOH solution = 3.21 ×10 -2 M  pH of a 3.21 ×10 -2 M solution of KOH = ?…

Q: Determine the [H*], [OH-, and pOH of a solution with a pH of 10.33 at 25 °C. [H*] = M [OH] = РОН 3…

A: Given data is as follows: The pH of the solution = 10.33 The pH of a solution can be calculated as…

Q: 37. A solution has a pH of 10.65. What is the [H3O+] value for this solution?\ a. 2.2 x 10-11 b. 4.5…

A: In Chemistry, pH is a scale which is used to specify the acidity or basicity of an aqueous solution.…

Q: A solution has a pH of 8.0 at 25°C. What is the hydroxide-ion concentration at 25°C? O a. 8 M O b.…

A: pH is the negative logarithm of H+ concentration to the base 10 represented by: pH = -log H+ For a…

Q: Determine the [H*], OH-], and pH of a solution with a pOH of 2.72 at 25 °C. [H*] = M [OH"] = M pH =

A: Given value-> pOH = 2.72

Q: What is the pH of a 7.49 × 10-3 M HI solution? Is the solution acidic, neutral, or basic? acidic…

A: As we know that, pH < 7 Acidic solution pH = 7 neutral solution pH >7 basic solution

Q: 13. If the pH of a 0.45 M ammonia solution is 11.73, what is the ionization percent of the base? А.…

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

Q: Q2// Calculate the pH for o.2M Ammonium acetate, the ionization constant for Acetic acid and…

A: Given : Concentration of Ammonium acetate = 0.2 M Ionization constant = 1.8 × 10-5

Q: 8. An unknown solution has a [H*] (acid concentration) of 2.8*105. Calculate the pH and pOH of the…

A:

Q: neutral ? II maintain its pH. Solution is acidic, basic, or neutral? [H3O+ ] [ОН-1 PH 4.56 x 10-2…

A:

Q: what was the pH of the AOm(OH)m unknown aqueous solution? The hydrogen ion concentration of the…

A: Given Hydogen ion concentration of unkown solution is [H+] =1×10-5m We have to calculate the ph of…

Q: What is the pH of a solution with H306 M? A 5.8 b. 11.0 C.6.2 12. 4.3

A:

Q: If [H*] of a solution is 0.001 M, pH of the solution is Select one: O a. 3 Оb. 14 О с. 10-3

A: We have given that Concentration of H+ solution is given by [H+] =0.001M = 10-3M pH = -log[H+]

Q: What is the [H3O+] if pH = 7.45?

A: Since the pH of any solution is given by  pH = -log[H3O+] where [H3O+] = concentration of H3O+ ions…

Q: The pH of a solution is 9.65. The solution is Land the hydroxide concentration is than the hydronium…

A:

Q: The hydrogen ion concentration is 1 x 10-6. What is the pH of the solution? -8 a O b -6 6 O d 8

A: pH is a measure of H+ ion concentration→ the higher the H+ ion concentration, the lower the pH (i.e.…

Q: A cup of coffee has a hydroxide ion concentration of 1.0 x 10-3 M. What is the pH of this coffee? O…

A: First option. A. 11

Q: Calculate the pH of a HNO3 solution with a hydrogen ion concentration of .25M A. 0.56 B. 0.6 C.…

A: Given, [HNO3] = 0.25M

Q: Calculate the pH of a 0.10 M NaBrO solution. (a) 3.22 (b) 10.78 (c) 11.02 (d) 9.96

A: NaBrO is a salt of strong base NaOH and weak acid HBrO. The pH can be calculated using the following…

Q: Calculate the pH of a solution if the concentration of H+ is 2.67 x10^(-5)M A. 11 B. 4.57 C. 7M…

A:

Q: Hydrazine, N2H4 has Kb= 1.3E-6. Calculate the pH of 0.486M solution of N2H4.

A: Hydrazine is a weak base.We have to calculate pH given hydrazine solution. Recall the following…

Q: What is the pH of the following solution? 3.9*10^-5 M H3O- at 25 degrees Celsius  A) 5.41 B) 8.59…

A:

Q: The pH of a solution of Ba(OH)2 is 10.95 at 25 °C. a What is the hydroxide ion concentration in the…

A: Given  PH of a Ba(OH)2 solution =  10.95 Hydroxide ion concentration = ?

Q: 6.7

A: Here : O.35 M = C ( original concentration )  [H+] = √( Ka1 • C )  Using this formula, Calculate…

Q: What is the pH when the hydrogen ion concentration is 1 x 10^-12 M? O a) -2 O b) -12 O c) 12 d) 2

A: Given : Hydrogen ion concentration i.e [H+ ] = 1 X 10-12 M

Q: What is the pH of a 5.737E-12 molar OH solution? (pOH = -log[OH ]and pH + pOH = 14) %3D

A: pH of a solution is used to identify whether the solution is acidic or basic in nature. The pH of…

Q: A solution with (OH- )of 5 x 10^3 has a pH of? A.-2.3.   B. 11.7.   C 7.0. D. 2.3

A: (b) 11.7 Concentration of OH- ions = 5×10-3 Now, pOH = -log[OH-]                    = -log (5×10-3)…

Q: Question attached

A: pH of solution is measure the acidity or basicity of solution and it calculated by the following…

Q: What is the pH of a 0.200 M solution of HNO3?   0.70   1.31   6.18   8.53

A:

Q: 1. Calculate the pH of the following: a. [H*] = 1 x 10³ M %3D b. [OH]=1 x 10$ M C. [H]=1 x 107 M

A: Calculate pH of the given data---

Q: The pH of a solution is 5.93. Find the pOH, [H;O*], and [OH-].

A:

Q: Which of the following HCO(3)- to H(2)CO(3) ratios represent(s) an acidic pH? 1. 18:1 2. 28:1 3.…

A: The ratios 18:1 and 12:1 between bicarbonate ions (HCO3-) and carbonic acid (H2CO3) represent an…

Q: Determine the pH of 1.5 M HBrO. (Ka HBrO = 2.5 x 10–9)

A:

Q: The PH of a solution containing a [H3O+]= 3.40 x 10 -5 M, is: a. 1.67 b. 3.40 c. 4.47 d. 12.3

A: Given : [H3O+ ] = 3.40 X 10-5 M

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.