The pain reliever codeine is a weak base with a Kb equal to 1.6×10–6. What is the pH of a 0.250 M aqueous codeine solution?

Q: What is the pH of a 8.47×10-2 M aqueous solution of sodium acetate, NaCH3COO? pH =  This solution…

A: Given- Concentration of sodium acetate (NaCH3COO) aqueous solution = 8.47×10-2 M a Concentration of…

Q: We can ignore the contribution of water to the concentration of OH− in a solution of the following…

A: Concept introduction: A weak base can ionize partially to form OH- ions and respective anion. The…

Q: 1. Are food items such as juice or vinegar acidic or basic? What ion probably accounts for this…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What is the pH of a bleach solution that has a [OH−]=5.6×10−6 M?[OH−]=5.6×10−6 M? pH=pH=     Is…

A:

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid.   What is the pH of a…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: What is the pH of a solution that is 2.7×10-9 M in NaOH

A:

Q: *please help with question 8b*** 8. A certain brand of antacid uses calcium carbonate to neutralize…

A: pH = -log[H+][H+] = 10-pH Given,  pH of gastric acid = 0.9 H+ = 10-0.9H+ = 0.1259M

Q: What is the pH of a 6.2 x 10-5 M NaOH solution?

A:

Q: 10. What is the pH of a 0.4M ammonia solution? The ionization constant of ammonia is 1.8 X 10.

A: Given: Concentration of ammonia solution = 0.4 M Kb of ammonia = 1.8×10-5

Q: Rainwater that falls close to a power plant has H3O+ ion concentration of 6.25x10-4. What is the…

A: Formula of pH  pH = -log[H+] or pH = -log [H3O+]

Q: What is the pH of a 1.5x10-7 NaOH solution?

A: Given , Solution is NaOH Molarity = 1.5×10-7  { I am considering the the solution expressed in…

Q: If the OH- ion concentration of a blood sample is 4.7 ×10−7 M, what is the pH of the blood sample?

A: We know that, pOH can be expressed as the negative logarithm of hydroxide ion concentration, i.e.…

Q: If a solution of aspirin has a [OH-] = 4.4 x 10–12 M, what is the pH of the solution?

A: Given, [OH-] = 4.4 ×10-12 pH is the negative logarithm in hydrogen ion concentration.

Q: The pH of a basic solution is 11.99. What is [H⁺]

A: pH of the solution  is defined as "the negative logarithm to the base 10 of the value of the…

Q: What is the pH of a solution made by diluting 24 mL of 0.12 M HClO4(aq) to a total volume of 250 mL?

A: pH is the negative log of H+ concentration .  Upon dilution H+ concentration decreases . And also pH…

Q: The pain reliever codeine is a weak base with a K, equal to 1.6x10-6. What is the pH of a 0.05 M…

A: pH of a solution is defined as the negative  logarithm of H+ ion concentration. Given codeine…

Q: For the reaction below, which substances are bases according to the Brønsted-Lowry definition? HOBR…

A: a) Species which can accept a proton is called Bronsted - Lowry base . Also lone pair of electrons…

Q: What is the approximate pH of a 0.02 M solution of a strong monoprotic acid? Of a 0.02 M solution of…

A: Molarity of monoprotic acid=0.02MMolarity of Strong base(KOH)=0.02M

Q: The hydronium ion concentration in blood of three different patients was:  Patient    [H3O+]…

A: pH = - log [H3O+] Patient 1 pH = - log [7.94 x 10-8] = 7.1 Patient 1 has an abnormal blood pH.

Q: Use the concentrations of [H3O*] and [OH] to calculate the missing concentration and indicate…

A: When the concentration of OH- is given, pOH is calculated. And when the concentration of H+ is…

Q: What is the pH value of the solution formed by mixing equal volumes of a strong acid solution with a…

A:

Q: What is the pH of a cleaning solution with a  [H30+]= 7.4 × 10^9M  [H3O+]

A: To calculate the pH of a cleaning solution to following calculation is used

Q: One aqueous solution of a strong acid has pH = 1.20, another pH = 1.80. If equal volumes of these…

A: First find the H+ concentration of both the solutions and find H+ concentration after mixing the…

Q: An aqueous solution contains 0.050 M HCl at 25.0 °C. What is the pH of the solution?

A: The pH of the solution can be calculated as follows -

Q: What is the pH of a 1.5 M solution of NaNO2?

A: Molarity of NaNO2 = 1.5 M

Q: What is the pH of a urine sample that has an H 3O + concentration of 1 × 10 −5 M? Classify the…

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

Q: 6.)Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.

A:

Q: at 0.125 M aqueous solution of a weak base is 9.2% ionized. what is the pH of the solution?

A: Given  Concentration (c) = 0.125 M Percentage ionization = 9.2 % pH = ?

Q: What is the pH of a 8.4 x 10–5 M Ba(OH)2 solution?

A:

Q: Calculate the pH of an aqueous solution of 0.2100 M potassium carbonate. pH

A:

Q: Assuming complete dissociation, what is the pH of a 4.04 mg/L Ba(OH)2 solution? pH=

A: Given :  We have to calculate pH.

Q: Which solution below has the highest concentration of hydroxide ions? pH = 8.2 pH = 5.6 pH = 3.7 pH…

A:

Q: Propionic acid, C2H5CO2H (Ka = 1.34 × 10−5), is used in the manufacture of calcium propionate, a…

A: pH means "potential of hydrogen" which is a scale used to specify the acidity or basicity of an…

Q: Calculate the following for the given aqueous solutions at 25.0 oC:​a) The [H+] concentration of an…

A: Given a)  pH = 1.02 ( as pH cannot be negative ) b) Concentration of HNO3 = 7.27 × 10-8 M

Q: Which of the following is an Arrhenius base? A KNO, 3. B H,SO, CHO 6 12 6 D КОН

A:

Q: A 1.23M solution of an unknown weak base has a pH of 11.5. What is its Kb?

A: pH of the week base = 7+0.5×pKb +0.5×logC

Q: 3. Which is an example of an acid? A. NH3 C. NaCl B. NaHCO D. CH3COOH 4. Which one of the following…

A: 3) acidity depends on two factor- i) donation of H+ ion. ii) stability of conjugate base. Here…

Q: The pain reliever codeine is a weak base with a Kb equal to 1.6x10-6. What is the pH of a 0.05 M…

A: Formula of pH of weak base is pH = 14 - (1/2) pKb + (1/2) log C Here C = concentration of weak base…

Q: 16.82 Brown) Using data from appendix D (or any online weak acid table), calculate [OH-] and pH for…

A: (1)  F-+H2O  ⇌ HF + OH-concentration F- = 0.105 MKa = 6.8×10-4Kb = KwKa = 10-146.8×10-4 =…

Q: The pH of an aqueous solution of 0.483 M nitrous acid is

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: Calculate the pH of a 7.4 x 10–4 M solution of Ba(OH)2.

A: We will Calculate pH.

Q: The pH of an aqueous solution that contains 3.4 x 10-2 M NaOH is ______

A:

Q: The pH of a 0.10 M solution of a weak base is 9.67. What is the Kb of the base?

A: Assuming the weak base is monoprotic base Hence the dissociation of base will have below reaction…

Q: Aniline, C6H5NH2, is a weak base with Kb = 4.2 x 10–10.  What will be the pH of a 0.188 M aniline…

A: Given, kb = 4.2 x 10-10 molarity = 0.188 M  PH = ?

Q: Potassium hydroxide is classified as a base because KOH contains O a K* ions O b 0²- ions OH- ions O…

A: Given here potassium hydroxide is classified as a  base.we are asked to choose option in the given.

Q: What is the pH of an aqueous solution made by combining 43.55 mL of a 0.3692 M ammonium chloride…

A: Ammonia, NH3(aq) is a weak base and ammonium chloride, NH4Cl, or NH4+(aq) is a conjugate base of…

Q: Which of the following forms a solution with a pH of 13?        A. 0.01M solution of NaOH   B. 0.03M…

A:

Q: The pH of a weak base (B) is 9.99 when the concentration of the weak base is 0.18 M. What is the…

A:

Q: 500.0 mL of HCl gas at 27∘∘C and 750.0 mmHg completely dissolves in 100.0 mL of pure water, what is…

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.