Calculate the concentration of each species present in a 0.050-M solution of H2S.

Q: 2. One mole of H* is always neutralized by mole of OH-.

A: -> If water form from combination of ions  then it is neutralization .

Q: How would you categorize a solution that has a concentration of hydroxide ions equal to 3 x 102 M? O…

A: A solution is acidic if pH<7 Basic if pH>7 Neutral if pH=7 pH is the -log[H+] pOH = -log[OH-]…

Q: Determine the [OH-] concentration in a 0.235 M NaOH solution.

A:

Q: What are [H+] and [OH-] in a 0.344 M solution of HNO3

A: HNO3 is a strong acid and hence, it dissociates completely into its ions. And the concentration of…

Q: Calculate the concentration of all species in a 0.15 M KF solution.

A: The constant Kb denotes the ionization of a base. The smaller the value of Kb for a base, the weaker…

Q: a solution has a concentration of OH- =4.0x10-5 M. what are the concentration of H3O+ and the pH of…

A: pH of a solution can be defined as negative of logarithm of concentration of hydronium ions

Q: Find the pH of a 0.010 M HNO2 solution.

A: HNO2 is a weak acid with dissociation constant, Ka = 7.2 X 10-4  Hence HNO2 will dissociate…

Q: Rank the solutions in order of decreasing [H3O+]: 0.10 M HCl;0.10 M HF; 0.10 M HClO; 0.10 M HC6H5O.

A:

Q: What is the pOH of an aqueous solution that has a hydroxide ion concentration of 7.0 ✕ 10−4 M?

A: POH  = -log (OH-)

Q: Calculate the pH and [OH'] of a 0.001 M solution of NaOH.

A: Given :- molar concentration of NaOH = 0.001 M  To calculate :- [OH-] and pH of the solution

Q: Calculate the pH and the concentrations of all species in a 0.1500 M NH4NO3 solution.

A:

Q: Calculate the concentration of all species in a 0.155 M solution of H2CO3.

A: Given - H2CO3 = 0.155 M To find - concentration of each species

Q: Calculate the concentration of H30* in a solution that contains 1.8 x 10° M OH at 25°C. Identify the…

A: Given :- [OH-] = 1.8 × 10-5 M  To calculate :- [H3O+] and nature of the solution    Since you have…

Q: Suppose 0.5 L of a HNO3 solution has a pH of 2.20. How many moles of HNO3 must have been initially…

A: pH = -log[H+]  where [H+] = concentration of H+ ions  Hence substituting the values we get  2.2 = -…

Q: Calculate the pH of a 0.015 M solution HBr .

A: Strong acid:The solution that is completely dissociates into its ions in water. This makes to…

Q: Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution

A: Construct ICE table and calculate the required values,

Q: Calculate the [H3O+] and pH of a 0.62M NaOH solution.

A: Given, Concentration of NaOH = 0.62M

Q: Calcium hydroxide is a strong acid Oweak acid strong base O.weak base O neither acid nor base

A: • We need to determine the nature of calcium hydroxide.    • The formula of calcium hydroxide is…

Q: Convert 0.035 M OH- concentration to pH value (in aqueous solutions).

A:

Q: What are [H+] and [OH-] in a 0.00338 M solution of KOH

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the OH⁻ concentration in this solution 1.05 M C₅H₅N?

A:

Q: What is the pH of a solution with a concentration of 0.00001 moles/ml (M) of H1?

A: Gvien, concentration of 0.00001 moles/ml (M) of H1

Q: What is the theoretical pH of a 0.00001 M HBr solution?

A:

Q: Calculate the concentration of all species in a 0.500 M solution of H2SO3.

A:

Q: Show the calculation required to determine the pH of a solution that has H3O+ concentration of…

A: pH of solution is defined as negative logarithm of hydrogen ions.

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the [H3O+].

A: Given: The concentration of hydroxide ions is provided,i.e. [OH-] = 1.0 x 10-5 M. The hydronium ion…

Q: What is the pH of a 0.005 M aqueous HCl solution?

A: Given, concentration of HCl = 0.005 M HCl is a strong acid . It dissociates Completely in aqueous…

Q: What is the pH of a 0.00810 M solution of HCl?

A: pH of a Solution pH of a solution can be determined by the following formula pH = -log[H+ ] Where…

Q: For a solution with a hydroxide (OH-) concentration of 5.0 x 10-5 M, what is the concentration of…

A:

Q: Determine the molar concentration of each ion in 0.025M solutions of the following compound. KOH

A: Strong electrolytes are those electrolytes which dissociate completely in the aqueous solution. The…

Q: Calculate the concentration of all species in a 0.380 M solution of H3SO3

A: Solution: Concentration (Molarity) of S = 0.380M Concentration(Molarity) of H = 1.14M…

Q: What is the concentration of ion or molecule in the solution of 0.25 M NaNO3?

A: Given,0.25 M NaNO3

Q: Question is attached

A: Given information: Concentration of dimethylamine = 0.393 M

Q: Calculate the percent ionization of a 0.520 M solution of phenol (a weak acid), C6H5OH. %…

A: The given data is as follows: The concentration of phenol = 0.520 M The percent ionization of phenol…

Q: Calculate the concentration of OH- in a 0.15 M solution of NH3.

A:

Q: What is the pH of (a) a 0.028 M solution of NaOH

A: Given: Concentration of NaOH=0.028M To find: The pH of the solution

Q: What are the concentrations of H+ and OH− in a solution of 150 mM HCl?

A: Conc. of given HCl Soln  = 150 mM  (Since 1 M = 1000mM )  = 0.15 M   H+ + Cl- ---> HCl  As we can…

Q: What concentration of NH4NO3 is required to make [OH−] = 1.0 × 10−5 in a 0.200-M solution of NH3?

A: It is given that the [OH-] in a 0.200 M solution of NH3 is 1.0 ×10-5 and the concentration of NH4NO3…

Q: The pOH of an aqueous solution of 0.592 M aniline (a weak base with the formula C6H5NH2) is

A:

Q: What is the pH of a 0.00670 M solution of HCl?

A: pH = -log [H+]

Q: Calculate the concentration of H+ ions in a .62 M NaOH solution

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

Q: Calculate the pH of a 0.00118 M solution of HBr.

A: Given data contains, Concentration of HBr is 0.00118 M. Hydrobromic acid is a strong acid so it gets…

Q: Calculate the concentration of H* ions in a 0.62 M NaOH solution.

A:

Q: Determine the concentration of OH- and H3O+ in a 0.0123 M solution of sodium cyanide, NaCN.

A:

Q: Household ammonia is a solution of the weak base NH3 in water. List, in order of descending…

A: To arrange all the ionic and molecular species present in a 1-M aqueous solution of weak base NH3

Q: Calculate the pH of a 0.00015 M NaOH solution. NaOH is a strong base and completely dissociates in…

A:

Q: If it takes 25 mL of 0.25 M H2SO4 solution to completely neutralize 100 mL of potassium hydroxide,…

A: 25 mL of 0.25 M H2SO4 solution to completely neutralize 100 mL of KOH. At neutralization point :-…

Q: What is the hydrogen ion concentration, pH, and pOH of a solution with a hydroxide ion concentration…

A:

Q: The hydronium ion concentration in an aqueous solution at 25 o C is 6.1 × 10-2 M. What is the…

A: Given- Hydronium ion concentration= 6.1×10-2M Hydroxide ion concentration=?

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.