B. If the pH of a weak acid solution is 2.500 and the solution has a concentration of 0.100M, what is the Ka of the weak acid HA?

Q: Methylamine, CH3NH2, is a weak base.CH3NH2(aq) + H2O(ℓ) ⇄ CH3NH3+(aq) + OH−(aq)If the pH of a 0.065…

A: Given data contains, pH=11.70 Concentration is 0.065 M. The pOH is calculated as, The pOH is 2.30.

Q: Using the data table write th formula of the conjugate base that has the weakest base?    Acid…

A: Bronsted-Lowry acid-base theory: According to the Bronsted-Lowry acid-base theory, acid is a…

Q: Determine Kb of the weak base B whose conjugate acid HB+ has Ka 6.5 × 10−4.    × 10    Determine the…

A: The Ka and Kb are related as,

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

A: The pH is used to determine the alkalinity or acidity of a solution. The pH is given as the negative…

Q: Which acid is the weakest? O :CI-0-H O :0=C-0-H O. :0: :0=CI–0-H :0: :0=CI-0-H :0:

A: strength of the inorganic acids can be determined using their structure and elements present into…

Q: 4. If 0.25 M of an acid (HA) has pH = 5.73, which of the following statements is true about this…

A:

Q: An unknown weak acid with a concentration of 0.077 M has a pH of 1.80. What is the Ka of the weak…

A: The Ka of weak acid

Q: What fraction of HA dissociated? If the total concentration of acid (= [HA] + [A'] is 0.060 M and…

A: In order to solve this question, we must know that the reaction is at equilibrium and under chemical…

Q: What is the pH of 0.0015 M NaOH?

A: NaOH is a basic and it is a strong base because it is a strong electrolyte and it will dissociated…

Q: Glycolic acid ionizes in water with a Ka value of 1.5x10-4           HOCH2COOH +H2O ⇌ H3O+ +…

A: Given:   Glycolic acid is a monoprotic acid. The concentration of glycolic acid is 0.90 M.

Q: A strong acid has a large or small Ka value?

A: Strong acid is a type of acid which has a high tendency to dissociate into ions in the aqueous…

Q: Kraakenoic acid, when dissolved in 25 °C water, has a Ka of 6.66x10-6.  What is the Kb for the…

A: Relation between Ka and Kb , at 25 degree celcius  Kw = Ka * Kb

Q: Determine the Ka of a weak acid HA that has a concentration of 0.025 M and a pH of 4.09 at 25°C.

A:

Q: If its volume is 500 mL and its contents have a pH of 2, how many moles of H does it contain? ffgurn

A: To solve this problem first we have to calculate the concentration of H+ ion  then we will calculate…

Q: e) Compare the pH of two basic solutions (0.1mM & 100mM NaOH). As base becomes more diluted, does…

A: Working formula pH = - log [H+] and pOH = - log [OH-] pH + pOH = 14

Q: An unknown weak acid with a concentration of 0.130 M has a pH of 5.600. What is the Ka of the weak…

A: Assuming the unknown weak acid is HA Hence the dissociation reaction of acid is  HA ------> H+ +…

Q: Calculating the PH UI A solution is prepared at 25 °C that is initially 0.45M in ammonia (NH,), a…

A: Initial concentration of ammonia=0.45M  Concentration of ammonium chloride=0.13M  Kb=1.8×10^-5 pH of…

Q: 2. Determine the pH if I add 0.5 moles of NHẠC1 (s) to a 5 L solution of water. (Note: the Ka of…

A:

Q: How many times greater is the [H+] in coffee than in neutral water if the pH of coffee is…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Based on the given Ka values, which is the weakest base? Acid Ka CH3COOH 1.8 x 10–5…

A: Equilibrium constant (K) is ratio of concentration of products and reactants. Addition or removal of…

Q: Determine the Kb of a weak base that has a concentration of 0.75 M and a pOH of 4.74 at 25°C.

A:

Q: The pH of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

A:

Q: solution that shows a pH of 11.70 has a  [H+] of what?

A:

Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

A:

Q: An unknown weak acid with a concentration of 0.085 M has a pH of 1.80. What is the Ka of the weak…

A:

Q: If the ph of 0.10 M HA (weak acid) is 4.10, calculate Ka for this weak acid.

A: From given pH value the hydronium ion concentration is determined first.

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.230 M  solution of methylamine?

A:

Q: What mass of HNO3 is needed to make 315.0 mL of a solution with a pH of 2.27?

A: Consider the given information is as follows; Volume of the solution = 315.0 mL = 0.315 L…

Q: Calculate the pH of a 0.0644 M anilinium chloride solution. pH= Calculate the concentrations of…

A: Let us consider a ICE table below, HA = conjugate acid = 0.0644 M (anilinium chloride ) A- =…

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

A:

Q: If the pH of lake water falls below 5.0, it is considered as “dead”. Taal lake has a concentration…

A: The question is based on the concept of PH calculations. we have been given pOH of the lake. we need…

Q: Determine the [H+], [OH-], and pOH of a solution with a pH of 6.81 25 ° C.

A:

Q: Which would have a more basic pH, a solution whose hydrogen ion concentration is 1.0 x 10^-12 M or a…

A: We know that pH is the negative logarithm of the concentration of Hydrogen ion.  pH = - log [H+] And…

Q: : Find the Kw of pure water at 50.0°C, if the pH is 6.630? 2: Find the pOH in an aqueous solution…

A:

Q: HX is a weak acid: Ka = 5.52 × 10–7. Calculate the pH of a solution in which [HX] = 0.0501 M and…

A: Here HX is a weak acid. Given data, Ka =5.52×10-7 [HX]=0.0501 M and [X1-]=0.00845 M

Q: if the H3O+ ion concentration in an aqueous solution at 25 °c measured 4.61 * 10^-8 M, what is the…

A: Given : [H+] = 4.61 * 10^-8 M

Q: What is the pH of NaOH that has a concentration of 0.013 M?

A: NaOH is a strong base and dissociates completely as Na+ and OH- in solution. As it dissociates…

Q: At 40°C and 1.00 atm pressure, a gaseous monoprotic acid has a density of 1.05 g L-1 . After 1.85 g…

A: Given: Temperature =  40°C = (273+40) = 313 K pressure = 1.00 atm density = 1.05 g L-1 mass of gas…

Q: Calculate the pH of an 0.025 M solution of HF. HF is a weak acid Ka = 0.00071

A: The PH of weak acids can be calculated as follows

Q: If a weak acid  (HA) has a Ka of 1.35 x 10-8, what is Kb for A-, the conjugate base.

A: If a weak acid (HA) has a Ka of 1.35 x 10-8, the Kb for A-, the conjugate base is to be calculated.

Q: A particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar…

A: Given : Acetic acid solution (i.e vinegar) with pH = 2.90  Ka of acid = 1.8 X 10-5  The dissociation…

Q: HIO3 has a ka of  0.16. What is the pH of a 0.600 M HIO3 solution? (use successive approximations)

A: The strength of an acid depends on the extent of its dissociation in water. Strong acids dissociate…

Q: What is the pH of a solution of a 0.045 M of a strong acid? (1.35

A:

Q: The pH of a 0.30 M solution of an acid, HA, has a pH = 5.20. Calculate Ka of HA

A: To calculate Ka of HA: The dissociation constant for the acid:

Q: In water, the amphoteric ion HCO3 will act as x 107, 4.8 x 10 11 Ka values for H,CO3 are 4.3 an acid…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: What is the H,O"| of a solution of HI with a pH = 1.45? O la) 0.0355 O (b) 0.1173 O (c) 0.3548 O (d)…

A:

Q: Calculate the H3O+ concentration from each pH: (a) 4

A: We know that,the relationship between pH and concentration of H3O+ is- pH=-log(H3O+) where, the…

Q: The Ka for HC2H3O2 is 1.8 x 10-5. What is the pH of a 0.02M solution of this weak acid?

A:

Q: Calculate the pH of a 0.10M weak acid, HA, whose Ka is 1.8 X 10

A: Given that: Concentration of weak acid,(HA) = 0.10M Ka = 1.8×10-5 Weak acid partially dissociates…

Q: What is the pH of a 0.25 M solution of a strong acid?

A: The Formula of pH of solution is        pH = -log10[H+]

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.