What is the pH of a 75.0 mL solution that is 0.043  M in weak base and 0.059 M in the conjugate weak acid (Ka=7.2×10^−8)?

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: What is the pH of a 75.0 ml of a 0.1 M pyridine (C5H5N) solution (Kb= 1.7 x 109) when 100.0 mL of a…

A:

Q: Acetic acid (CH, COOH, K, = 1.80 x 10-) is a weak acid, so the salt sodium acetate (CH, COONA) acts…

A: Given, Ka = 1.8 × 10-5 , [CH3COONa] = 0.566 M The reaction : CH3COONa + H2O ⇔  OH- + CH3COOH

Q: The pH of an aqueous solution of 0.415 M aniline (a weak base with the formula C,H&NH,) is

A:

Q: The pH of a 1.00 × 10² M solution of cyanic acid (HOCN) is 2.77 at 25.0 °C. Calculate Ka for HOCN…

A: Solution :         The process of dissociation involves the segregation of molecules into smaller…

Q: 5) a) Calculate the pH of 5 liters, 1.00 M HA weak acid solution. (Ka= 6.8 x 10*) Calculate the…

A: 5 a. Given: Ka = 6.8×10-4 Initial concentration of HA = 1.0 M

Q: Enter your answer in the provided box. Determine the K, of a weak base if a 0.29 M solution of the…

A: The pOH of 0.29 M solution is calculated below.

Q: Calculate the pH of 50.0 ml of 0.250 M oxalic acid (HOOCCOOH) upon addition of 15 mL of 0.500 M…

A: Oxalic acid is a diprotic weak acid, whereas monoacidic NaOH is a strong base. Given the volume of…

Q: 1    Calculate the pH of a 0.02 M solution of the weak acid, HA.         Ka = 2.46 X 10 –4…

A:

Q: What is the pH of a solution prepared by dissolving 3.00 g of the weak acid HA (molar mass- 138.12…

A: pH of the solution indicates that the solution is acidic or basic in nature.  If the pH of the…

Q: What is the pH of a 0.677 M weak base solution? The K_{b} of the weak base is 0.000017.

A: we need to calculate the pH  0.677 M weak base solution

Q: Butyric acid, C3H,COOH, has ionization constant of 1.54 x 105. a) Calculate the pH of 50.0 mL of a…

A: part C pH of the resulting solution can be calculated using the values of volume and molarity of the…

Q: Calculate the pH of a 0.0010 M solution of HB, a hypothetical acid with K-9.6 x 10. (Use the method…

A: The pH of 0.0010 M HB solution is calculated as shown below. H+=KaC=9.6×10-5×0.0010 M=3.10×10-4 M

Q: What is the pH of a solution that contains 0.10 M cyanic acid and 0.20 M sodium cyanate?

A:

Q: Consider the following ions: Cl-, HS-, NO2-, F-, and HS04-. (a) Which of these ions in water gives…

A: Given ions  Cl- HS- NO2- F- HSO4-

Q: 2. At 25°C , find the pH of (a) an ideal, 3.7 x 10³ M HCl solution; (b) an ideal, 1.00 x 10° M HCl…

A:

Q: 1. Identify the following as acidic or basic, and write the corresponding Ka or Kb reactions and…

A: Acid is a substance which release H+ ions and base is substance which release OH- ions

Q: A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA…

A:

Q: Strychnine (in contaminated wine) may have been used to poison Alexander the Great.  Strychnine…

A: The solution is provided below:

Q: The pH of 30 cm^3 of an acidic solution is 2.89. Calculate the concentration of hydrogen ions and…

A:

Q: The pH of a white vinegar solution is 2.20. This vinegar is an aqueous solution of acetic acid with…

A: Concentration of H+ can be calculated as follows:

Q: How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic…

A: Given : Concentration of HCl = 12.0 M Volume of HCl solution = 10.0 mL And concentration of acetic…

Q: What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Sr(OH)2 with 50.00 mL of 0.400…

A: Strontium hydroxide and lithium hydroxides are strong bases. They dissociate completely in the…

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: Identify the following as acidic or basic, and write the corresponding Ka or Kb reactions and…

A: (a) HF is a weak acid.  the reaction is : HF (aq) + H2O (l) ---------> H3O+ (aq) + F– (aq) Ka…

Q: The Ka of a weak monoprotic acid is 1.13 × 10−5 . What is the pH of a 0.0885 M solution of this…

A:

Q: At 10°C, the ion-product constant of water, K w, is 6.88 × 10 –15. What is the pH of pure water at…

A: Autoionization of water takes place as follows: The product of the concentration of the hydronium…

Q: Given 100 mL of a 0.245 M solution of pyridine (C5H5N pKb = 8.77), what is the pH if 100 mL of 0.245…

A: when Acid and base mix in equal milliequivalent form salt

Q: To what volume should 100 mL of any weak 0.30 molar monobasic acid (HA) or mono-acidic base (BOH) be…

A: According to the Le Chatelier principle, adding water to equilibrium would cause equilibrium left to…

Q: What is the ionization constant of a weak acid [HA], when its conjugate pair has a Kb value of 4.4 x…

A: In the ionization of a weak acid HA, A- is produced as a conjugated base.  HAAcid →Ionization…

Q: A solution of acetic acid (Ka = 1.8 × 10‒5) has a pH of 2.65. What is the concentration of acetic…

A: Given information: Ka of acetic acid = 1.8 × 10‒5 pH is 2.65

Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5 What is…

A: Given: The Ka (acid dissociation constant) value of acetic acid is 1.76 x 10-5 The molarity of…

Q: Calculate the pH of an aqueous solution of 2.16x10 M sodium sulfite. pH =

A: The given concentration of sodium sulfite = 2.16 ×10-2 M The dissociation reaction of sodium sulfite…

Q: Calculate the ph of 0.350 M acetic acid whose ionization constant is Ka= 1.8x10-5

A: Given :-  concentration of acetic acid solution = 0.350 M  Ka = 1.8 × 10-5  To be calculated :-  pH…

Q: Explain how you determine the pH of 0.500 M HOCI (Ka = 3.6 x 10) www m

A: pH  = - log [H3O+] HOCl is a weak acid and doesn't undergo complete dissociation in solution. Thus,…

Q: The pH of an acetic acid (Ka = 1.75 x 10−5) solution is 3.14.  What is the concentration of acetic…

A: Given :-  pH of acetic acid solution = 3.14  Ka for acetic acid = 1.75 × 10-5  To be calculated :-…

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-1 Ка(нсоон) = 1.77 ×…

A: Given: Ka (HIO3) = 1.6 × 10-1 Ka (HCOOH) = 1.77 × 10-4 We have to calculate the pH of a mixture of…

Q: What is the pH of a solution which is 0.023M in weak base and 0.039 M in the conjugate weak acid (Ka…

A: This question can be solved using Henderson-Hasselblach equation. The equation is, pH=pKa+…

Q: The pH of an aqueous solution at 25.0 °C that contains 3.98x10-9 M hydroxide ion is 6.50. TRUE OR…

A: pOH = - log [OH-]  pOH= - log (3.98 × 10^(-9)) pOH = 8.4

Q: Find the pH of a 0.250 M NaC2H3O2 solution.

A: The dissociation reaction with ICE TABLE C₂H₃O₂⁻ + H₂O ⇄ HC₂H₃O₂ + OH⁻ I 0.250 C -x +x +x E 0.250-x…

Q: What is the pH (in two decimal places) of a 0.047 M solution of Sr(OH)2?

A:

Q: The pH of a 0.5 M aqueous solution of formic acid, HCHO2, at 25.0 °C is 2.0. What is the value of Ka…

A: pH tells us about the acidic or alkaline values of a solution. Dissociation of a weak acid depends…

Q: The K₂ of a weak monoprotic acid is 1.74 x 10-5. What is the pH of a 0.0939 M solution of this acid?…

A:

Q: Calculate pH of the following solutions: 0.25 M HNO3 in 0.065 M CH COOH (K.=1.75x10).

A: Solution: We know the common ion aslo affect on oH of the solution. Here first we need to draw an…

Q: 9. Determine the pH of a 0.085 M sodium formate salt solution at 25°C. Sodium formate is a basic…

A:

Q: Enough water is added to 0.35g of benzoic acid to make 1000 mL of a solution. What is the pH?…

A: Given: Mass of benzoic acid=0.35 g Volume of solution=1000 mL =1 L Ionization constant for benzoic…

Q: A 0.861 M solution of a weak base has a pH of 11.80. What is the base hydrolysis constant, K, for…

A: Hydrolysis constant Kb can be calculated by the following way .

Q: If the Ka of a monoprotic weak acid is 1.4×10−6, what is the pH of a 0.14 M solution of this acid?

A: Given information: Concentration of an acid = 0.14 M Ka of weak acid = 1.4×10-6

Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Kb for the acetate ion is determined as follows,

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

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.