Acrylic acid, whose formula is HC3 H3O2 or HO₂CCH=CH₂, is used in the manufacture of plastics. A 0.86 M aqueous solution of acrylic acid has a pH of 2.16. What is K₁ for acrylic acid? Ka =

Q: When 0.412 g of a weak base with Kb = 3.10 ×10-5 the base is dissolved in 1.00 L of solution, it has…

A: Assuming the molar mass is M  Hence moles of base = mass / molar mass = 0.412 / M And concentration…

Q: A scientist dilutes 50.0 mL of a pH 5.85 solution of HCl to 1.00 L. What is the pH of the diluted…

A: Given data,pH=5.85Volume of HCl=50mL=0.050LDilution=1.0LKw=1.0×10-14

Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: A chemist is performing a titration in order to determine the amount of lithium hydroxide, LiOH(aq),…

A: Answer:The number of moles of any species in a solution is equal to the product of its molar…

Q: The pH of a 0.0059 M solution of Ca(OH)₂ is

A: The objective of the question is to calculate the pH of a 0.0059 M solution of Ca(OH)₂. The pH of a…

Q: Ka for HOCl is 3.2 × 10-8. How much chlorine (g) must be dissolved in 2.0 liter of water so that…

A: Given data are as follows Chemical reaction Cl2(g) + H2O(l) ⇌ H+(aq) + Cl–(aq) + HOCl(aq) Ka for…

Q: Consider the aqueous solutions of two weak acids depicted in diagrams A and B. (a) What is the…

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

Q: Household bleach is prepared by dissolving chlorine in water. Cl2(g) + H2O(l) ⇌ H+(aq) + Cl–(aq) +…

A: Given information: Ka for HOCl = 3.2 × 10-8 Volume of water = 3 litres. PH = 2.51 Given equation:…

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is?

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

Q: What is the pH of a 0.20 M solution of potassium cyanide,  K+CN- (Ka (HCN) = 6.2 × 10−10)?

A:

Q: Can you please answer sub question A and B and show all of the steps to the solution please and…

A: In the above problem the solutions are buffer solutions So we will use Henderson Hasselbalch…

Q: Consider two solutions, solution A and solution B. 3H+4 in solution A is 250 times greater than that…

A: A solution has pHA  = - log [HA +]  and [HA +] is the concentration of Hydrogen in solution A . B…

Q: Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M…

A: The relation between pH and concentration of  acid and its conjugate base is calculated using the…

Q: What is the pH of the solution that results from adding 21.1 mL of 0.12 M HCl to 25.7 mL of 0.41 M…

A:

Q: The pH of an aqueous solution of 0.534 M methylamine (a weak base with the formula CH3NH2) is

A:

Q: The compound dimethylamine is a weak base like ammonia. A solution contains 0.263 M (CH3)2NH₂*…

A: answer :pH is the measurement of the acidity of the solution.As per the given solution contains,…

Q: The hydronium ion concentration of an aqueous solution of 0.43 M formic acid, HCOOH is  [H3O+] =…

A:

Q: What is the pH of a solution that contains 6.13 x 10–4 M OH–?

A: pH measures the acidity of the solution whereas pOH measures the basicity of the solution -

Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

A: Since you have posted a question with multiple sub-parts, we will solve first two subparts for you.…

Q: A 20.6 mL sample of 0.382 M diethylamine, (C₂H5)2NH, is titrated with 0.272 M hydroiodic acid. At…

A:

Q: The pH of a 0.154 M solution of a weak acid, HB, is 2.72. What is K, for the weak acid?

A:

Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

A:

Q: A generic base, B¯, is added to 30.00 L of water. The pH of the solution is found to be 9.05. What…

A: The hydrogen ion [H+] concentration in the solution having a pH of 9.05 is calculated as shown…

Q: The pH of a 0.206 M solution of a weak acid, HB, is 2.59. What is K, for the weak acid?

A: pH = 2.59 pH = -log [H+]2.59 = -log [H+] [H+] = 10-2.59   Relationship between the dissociation…

Q: If 34.6 mL of a 0.68 M NaOH solution is added to a 51.9 mL sample of a 0.68 M weak acid, HA , what…

A: 34.6 mL of a 0.68 M NaOH solution is added to 51.9 mL sample of a 0.68 M weak acid, HA (ka = 1.8 x…

Q: QUESTION 7 7. Arrange the following compounds in order of increasing acidity. Explain. CH-CICO-H,…

A:

Q: It is believed that a bath in Epsom Salts can relieve various types of pain.  In preparation for…

A:

Q: Pyridine, C5H5N, is a bad-smelling liquid, that is also an excellent solvent. It is used to…

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: How many grams of sodium fluoride (NaF) need to be dissolved in 130 mL of a 1.56 M hydrofluoric acid…

A: The Henderson–Hasselbalch equation can be used to estimate the pH of a buffer solution.

Q: A solution of aqueous Ba(OH)2 has a measured pH of 12.462. What is the molarity of Ba(OH)2 in this…

A:

Q: A new potential cure for the common cold, code-named Z-123, is being tested by a pharmaceutical…

A:

Q: A solution contains 0.159 M sodium hypochlorite and 0.476 M hypochlorous acid ( K₁ = 3.5 × 10-8).…

A: Given that conc. of NaOCl = 0.159 M conc. of HOCl = 0.476 Ka of HOCl = 3.5 × 10–8 pKa = – logKa = –…

Q: The pH of a 0.0033 M solution of Ca(OH)₂ is

A: The negative logarithmic concentration of hydronium ions in solution is called pH. It is measured in…

Q: The pH of 0.01 M hydrochloric acid (HCl) is 2, the pH of 0.01 M sulfuric acid (H2SO4) is 1.7, and…

A:

Q: HCIO is a weak acid (Ka = 4.0 × 10-8) and so the salt NaClO acts as a weak base. What is the pH of a…

A:

Q: CO₂H 1. LiAlH4, ether 2. H₂O

A: Lithium Aluminum hydride is a strong reducing agent which can reduce carboxylic acids to alcohols.…

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

A:

Q: The pH of a solution for which [OH–] = 1.0 x10–6 is

A: Given:

Q: What is the pH of a solution prepared by adding 18.0 mL of 1.51 M nitric acid to 180.0 mL of 0.150 M…

A:

Q: The pH of an aqueous solution of 0.506 M methylamine (a weak base with the formula CH3NH₂) is

A:

Q: 4. In your chemistry laboratory class, you received a solution with an unknown pH. Find the pH of…

A: Concentration of NH3 = no. of moles/volume in Litre = 1/1 = 1M Concentration of NH4Cl = 0.4/1 = 0.4M

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.