What is pOH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10 Group of answer choices 9.07 4.73 4.93 9.27

Q: What is the concentration (in M) of H + ions in a solution at 25.0 °C with pH = 4.146?   a. 9.85…

A: Given: pH = 4.146 The pH of a solution is given by : pH =-log [H+]

Q: What is the pH of a 0.075 M LiF solution?  (Round answer to nearest decimal place.  Example, 75.877…

A:

Q: A solution that is 6.0×10−2 M in potassium propionate (C2H5COOK or KC3H5O2 ) and 8.0×10−2 M in…

A: A solution given is 6.0×10−2 M in potassium propionate (C2H5COOK or KC3H5O2) and 8.0×10−2 M in…

Q: Which of these solutions are basic at 25 °C?25 °C? Solution C: [H3O+]=5.57×10−4 MSolution C:…

A:

Q: 11. What is [H*] in M for a solution with POH=1 ]1 × 10–12 |1 x 10-7 1 × 10–13 |1 x 10-9 |None of…

A: PH is defined as negative logarithm of concentration of [H+] ion.

Q: Kb for NH3 is 1.8 × 10-5. What is the pOH of a 0.20 M aqueous solution of NH4Cl at 25.0 °C? A) 2.72…

A: NH4Cl is having the conjugate acid of NH3 i.e NH4+  Hence it will be ionised as per the reaction,…

Q: What is the pH of a 0.25 M weak acid solution with Ka = 5.4 × 10‒4? Group of answer choices   1.94…

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: Calculate either [H3O+] or [OH−]for each of the solutions.   Solution A: [OH−]=3.03×10−7 M; [H3O+]…

A: Given: Solution:A:  [OH−]=3.03×10−7 M; [H3O+] =   Solution B: [H3O+]=7.63×10−9 M; [OH−]=  Solution…

Q: The Ka for acid HA is 7.0 x 10-4. What is the pH of a 0.15 M aqueous solution of KA?   Answer…

A: pH is used to determine the concentration of hydronium ion.

Q: A diprotic acid (H₂A) has Kal = 4.28 x 10-7 and K₁2 = 5.45 x 10-¹1. What is the pH of a 0.431 M H₂A…

A: Firstly we find the concentration of H+ ion. Then we find the pH. Shown in step 2.

Q: If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic…

A: pH scale is basically used to determine the acidity and basicity of a solution. Like in general…

Q: 1. A1.0 M solution of a weak base B has a pH of 11.60. What is the valve of Kb for this base? а. 6.3…

A:

Q: Calculate the pH of a 0.15 M acid solution; Ka=2.95 x10-8 Group of answer choices 4.18 6.36 2.09…

A:

Q: What is [H30+] in a solution of 0.25 M CH3CO2H and 0.030 M NaCH3CO2? CH3CO,H(aq) + H20(1) = H30*(aq)…

A: Acetic acid and sodium acetate form buffer solution

Q: A 300 mL of 0.05M ammonia. The density of the solution is 0.88 g/mL. Pka pf ammonium = 9.255. What…

A:

Q: acid has a Ka of 1.8 x 10-5. Calculate the pH at the point when 30.00 mL of 0.150 M NaC2H3O2 is has…

A: The solution can be provided as:

Q: solution is prepared that contains 0.2 M HNO3 and 0.1 M HN3 (Ka=1.9x10-5). What is the concentration…

A:

Q: Which 0.10 M solution will have the largest concentration of hydroxide ion? a. NaHCO3…

A: b. NH3      (Kb of NH3 = 1.8×10–5)

Q: In which of the following aqueous solutions does the weak acid exhibit the highest percentage…

A:

Q: Calculate the Ka of a 0.400 M acid solution with [H30*]= 1.4x 10 4M O 1.40 x 106 O 1.40 x 10 5 O…

A: Equilibrium constant is defined as products concentrations divided by reactant concentrations to the…

Q: If the pKa of the indicator is approximately 6, to which of the following equivalence point will it…

A: Given, pKa = 6 At equivalence point,  pH = ?

Q: A solution of a weak acid contains 5 mM conjugate acid (HA), 2.5 mM conjugate base (A-), and 2.5 mM…

A:

Q: Find the percent ionization (?α) of a 3.0 M HNO2 solution. (Ka for HNO2 is 4.6 × 10-4) A) 1.2% B)…

A: Percent ionisation of HNO2 can be calculated as follows

Q: Calculate the following for both solutions [C2H3O2-]  [HC2H3O2] % ionization  Ka pKa 1.0 M HC2H3O2…

A:

Q: A solution has a [OH1-] = 4.20 x 10-4 M. Use the self ionization constant of water (Kw) to find the…

A: • The values provided in the question are:-    i) Hydroxide ion concentration of a solution, [OH-] =…

Q: A solution of ammonia is 3.2% ionized at 25.0°C. What was the original concentration (in M) of the…

A: It is given that ammonia is 3.2% ionized at 25°C and Kb is given as 1.8×10-5, the equation for…

Q: 7, Calculate the [H3O+] of a 0.110 M acid solution; Ka=5.45 x 10-7 Group of answer choices 4.55 x…

A:

Q: Which of the following statements is true about a 0.0100 molar sodium bicarbonate solution? The Ka…

A: Which statement is true

Q: What is the percent ionization of acetic acid (CH3COOH) in a solution that contains 0.10 M acetic…

A: Ionic solids are metal salts. They formed when metals form an ionic bond with non-metals. Ionic…

Q: What is the percent ioniation of 0.0550 M solution of HC2H202?

A: Strategy: Write the ionization equation and the expression for Ka. Next, find the concentration of…

Q: What is the [H3O+] of the blood if it has a pH of 7.4? What is the [H3O+] of milk if it has a pH of…

A: Interpretation-  To determine the [H3O+] of the blood if it has a pH of 7.4 and another determine…

Q: What is the [H+] in a 0.01 M Ba(OH)2 solution? Group of answer choices 1 x 10–2 M 5 x 10–13 M 1 x…

A: Since the base Ba(OH)2 will dissociate completely as => Ba(OH)2 ---------> Ba2+ + 2 OH-

Q: An unknown weak acid with a concentration of 0.057 M has a pH of 1.80. What is the Ka of the weak…

A: Given that: pH = 1.80 Concentration = 0.057 M Ka = ?

Q: Find the percent ionization of a 0.124 M weak acid solution whose KA  =  2.7 × 10–6. Group of…

A: Concentration of Acid (M) = 0.124M Also, Dissociation constant of acid KA=2.7×10-6

Q: Determine if the following salí solution is acidic, basic or neutral: NH4F GIVEN: Ka of NH4+ / NH3…

A:

Q: What is the pH when 20.0 mL of 0.10 M sodium hydroxide is added to 40.0 mL of 0.15 M HIO (Ka = 2.0 ×…

A: Given: 20 ml of 0.10 M NaOH (Base) 40 ml of 0.15 M HIO  (Acid) Ka of HIO = 2.0 x 10-11 we need to…

Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)? 2.770…

A: Given: Ka for CH3COOH= 1.75 × 10−5 The concentration of CH3COOH, (C) =  0.1055 M.

Q: Hydrofluoric acid has a Ka value of 7.2 x 10-4. What is the pH of a 0.040M solution of HF? a. 1.4 b.…

A:

Q: Calculate the pH of a 0.055 M solution of CH3COONa. (Ka(CH3COOH) = 1.8 x 10-5) Kw= 1.0 x 10-14…

A: [CH3COONa] = 1.8 × 10-5 Ka = 1.8 × 10-5 Kw = 1.0 × 10-14

Q: Which of the following statements is true about a 0.0100 molar ammonium chloride solution? The Ka…

A: Answer- We know that, salt of weak base and strong acid is acidic in nature.  ammonium chloride is…

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11.  What is the…

A: Given, concentration of HIO = 0.785(M) The equilibrium of HIO in aqueous solution is,  HIO(aq)…

Q: Calculate the [NH₃] in a solution of 0.480 M ammonium cyanide (NH₄CN). Hint: Use the Ka of HCN (4.9…

A: Answer is explained below.

Q: Calculate the percent dissociation of a 0.085 M solution of acetic acid, HC2H302. (ka=1.9x10)…

A: Formula  to calculate dissociation constant :

Q: Calculate the concentration of HC2H302 in a solution that is .12 M of NaC2H3O2. the Ka of HC2H302 is…

A: Given that: molarity of NaC2H3O2 = 0.12 M  Ka of HC2H3O2  = 1.8 x10 -6 To find:  the…

Q: Which of the following substances is NOT amphiprotic? Group of answer choices HPO42- NH3 HS− H2O…

A: The molecules or ions which can either donate or accept a proton are known as amphiprotic. Thus they…

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (CGH3O7)? CGH3O7(aq) +…

A:

Q: A 0.050 M solution of the weak acid HA has [H3O+] = 3.77 × 10-4 M. What is the Ka for the acid?

A: A form of equilibrium constant that measures the dissociation of acids and bases into its conjugate…

Q: The [H3O+] of a solution with pH = 2.0 is

A: The [H3O+] of a solution with pH = 2.0 is

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.