Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 x 10 M Select one: O a. 2.05 O b. 5.5 O c. 3.47 O d. 1.2

Q: The pH of a solution made up to contain 0.240 M H3PO4 and 0.480 M NaH2PO4 is- (Ka1= 7.11 x 10-3;…

A: Buffer solution are which can resist any change in PH when either acid or base are added and the PH…

Q: The following question refers to the following system: A 1.0 liter solution contains 0.25 M HF and…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: A solution with a low pH means what? 1. A high number of hydrogen ions are in a solution 2. A basic…

A: We are to find out what does a solution with lower pH mean. We will consider the concentration of…

Q: A solution with a pOH of 11.70 has an [H+] of a. 5.0 × 10−3 M.b. 3.2 × 10−4 M.c. 2.0 × 10−12 M. d.…

A: Given data, pOH of the solution =11.70

Q: 5.12

A: PH

Q: What is the hydronium ion concentration of 0.001 M NaHCO3 ? Select one: a. 8.3 b. 8 O c. 7.3 d. 8.8

A:

Q: At 25 degrees Celsius, what is the hydronium ion concentration in 0.100 M sodium chloroacetate? O a.…

A: Given,  Concentration of Sodium chloroacetate, ClCH2OONa is = 0.100 M

Q: The value of the ionization constant for a weak acid HA is 4.2 * 10 -7. What is the pH of a 0.35 M…

A: Given data ionization constant : Ka=4.2×10-7 Concentration of HA :  C=0.35 M   Now using the Ostwald…

Q: Find the hydroxide ion concentration of the solution with pOH= 1. a. 1.0x10-¹3 M b. 1.0x10¹¹ M c.…

A:

Q: 6. Hydrofluoric acid, HF, is a weak acid that dissociates in water according to the following…

A: We have to determine the conjugate base of HF in the given reaction

Q: The

A: Cl have more electronegative element than other so that it's Decreases the electrons charges density…

Q: The pH of a 0.50 M solution of the weak acid HA is 4.76. The value of Ka is O a. 6.0 x 10-10 O…

A: Given data :- Concentration of weak acid = 0.50 M pH of weak acid (HA) = 4.76

Q: Formic acid, HCOOH, is a weak acid with a Ka equal to 1.8×10 –4.  What is the pH of a 0.115 M…

A: Given: Ka is 1.8×10 –4 Molarity of formic acid is 0.115 M. Introduction: A weak acid dissociates…

Q: What is the pH of a 0.010 M solution of aqueous Sr(OH)2?   a. 10.2   b. 2.0   c. 9.0   d.…

A: To determine the pH of a basic solution, the pOH is determined first and then pH is calculated using…

Q: -5 Consider a 0.2M solution of CH3COOH (Ka = 1.8 × 10° M). Which ONE of the following is the correct…

A: The correct answer is given below

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: What is the K, of cinnamic acid if a 0.035 M cinnamic acid aqueous solution has a pH of 2.95? 4.44…

A:

Q: Calculate the pH of a 2.0 M Ca(OH)2 aqueous solution. a. 13.4 b. 14.3 c. 14.6 d. 13.7

A:

Q: Below are some properties associated with acid solutions and some properties associated with base…

A: Acids are sour in taste. Whereas bases are bitter in taste.

Q: The graph given below (Figure 1) shows [H+] vs. concentration for an aqueous solution of an unknown…

A: A) Since strong acids completely dissociates in solution producing H+ ions hence the concentration…

Q: The pH of a 4.6 x 10 -4 M Ca(OH) 2 solution at 25 °C is _____. Note that Ca(OH) 2 is a strong base.…

A: Given: The concentration of the Ca(OH)2 solution = 4.6 x 10 -4 M We have to calculate the pH of the…

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: A 0.25 M solution of a weak monoprotic acid has a hydronium-ion concentration of 3.5 x 104 M. What…

A: Concentration of weak monoprotic acid, [HA]  =0.25M [H3O+] = 3.5 X 10-4  M

Q: Determine the pH of 100.00 ml solution of 0.150 M oxalic acid following the addition of a. 50,00 ml…

A: The objective of the question is to determine the pH of the given cases.The pH is the measure of the…

Q: Question 11 Calculate the pH of a 0.30 M HNO3 solution. O 2.00 O 1.25 O 0.52 O 13.50 Question 12…

A: Given, [HNO3] = 0.30 M we know, HNO3 dissociate into one moles of H+ and one moles of NO3- which…

Q: The pk, for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.95 O b. 1.24 O c.…

A:

Q: The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10.  What is the pH…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: A given weak base solution is found to have [H+] = 4.3 x10-11 M. What is the [OH-] in this weak base…

A: In any aqueous solution at 25 degrees Celsius, the product of the hydrogen ion concentration [H+]…

Q: 13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82

A: The required equation is given below.

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: If the pH ofa solution is 3. ОА. 1.23х10 5м о в. 2.24х104м о С. 3.65х10"м D. 4.47x10-11м

A: pH of a solution - It is a measure of hydrogen ion concentration in a solution or can say a measure…

Q: 10. Calculate pH of a 0.45 M ammonia solution if the ionization percent is 1.2 A. 2.27 В. 1.57 С.…

A:

Q: The hydrogen ion concentrations in cheeses range from 1.00  10-5 M to 6.31  10-7 M. Find the…

A: pH = - log [H+]

Q: What is the concentration of H* ions in HCI whose pH is 8.3?

A: pH of the solution is equal to the negative logarithm of H+ ion concentration. Write the expression…

Q: What is the pH of .00055 M soln of NaOH?   A. 3.3 B. 1.3 E-3 C. 10.7 D. 1.55 E-7

A: Given  [ OH - ]   = 0.00055 M   PH         = ?

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: 3. If the H+ concentration in an aqueous at 25.0 C has a value of 0.100M, what is the pOH of the…

A: pH of the solution can be calculated as below:

Q: A 0.2 M sodium acetate solution is basic. TRUE or FALSE 2. The pH of 1.2 x 10-10 M HCl is equal to…

A: Sodium acetate is formed by the combination of a weak acid and a strong base. The mixture of a weak…

Q: Calculate the pH of a solution in which the molar concentration of H+ is 1.6 x 10-9. a. 1.60 b.…

A: Given information,     Molar concentration of H+ is 1.6 x 10-9.

Q: A solution has an OH- concentration of 1.0 x 10-3 mole/L. What is the solution's pH? a. 3.0 b. 4.0…

A:

Q: A given weak base solution is found to have [H+] = 4.3 x10-11 M. What is the [OH] in this weak base…

A: Step 1:     Option a is correct answer   Step 2: Step 3: Step 4:

Q: Which of the solutions listed below has the lowest pH?    A.  Pure H2O  B.  2.5 x 10-5 M HNO3  C.…

A: Lowest pH mean stronger acid and higher pH mean stronger base .

Q: What is the pH of 0.010 M aqueous hypochlorous acid? (K, of HOCI=3.5 x 10-8) a. 4.73 b. 7.45 c. 4.50…

A: The concentration of the hypochlorous acid is [HOCl]=0.010M Ka=3.5×10-8 pH=?

Q: What is the pH of a 0.040 M HNO 3 solution? A. 1.40 B. 1.70 C. 0.040 D. 12.30

A:

Q: In the reaction NH3  +  H2O  →   NH4+  +  OH–, the Bronsted-Lowry base is

A:

Q: What is the pH of a 0.379 M solutiôn of roxyla a. 0.42 b. 5.96 с. 3.19 O d. 6.38 O e. 4.2 x 10-7

A: Given, Molarity = 0.379 M Ka = 1.1 x 10-6  PH= ?

Q: A solution consists of 3.54x10^-9 moles of H^+ ions with a volume of 775mL. What best describes this…

A: To solve this problem we will use the formula  pH = -log[H+]   We also know that  If pH is less than…

Q: What is the percent dissociation of an acid given that the pH of a 0.30 M solution of benzoic acid…

A: Check the formula for the percent dissociation which contains molarity and pH is given 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.