What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x 10-10

Q: What is the pH of a solution that contains 0.10 M HCl and 0.10 M acetic acid (HC2H3O2)? Ka for…

A:

Q: What is the pH of an aqueous solution composed of 0.64 M NH4+ and 0.20 M NH3? (Ka of NH4+ = 5.6 ×…

A: Given: Molarity of NH4+= 0.64 M Molarity of NH3= 0.20 M

Q: What is the pH of a solution which is 0.021 M in weak base and 0.039 M in the conjugate weak acid…

A: We have a buffer system of weak base (0.021M) and conjugate weak acid (0 .039M) . We also have the…

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

A: Ka of HClO = 4.0 × 10-8 Concentration of the solution of NaClO = 0.089 M pH =?

Q: What is the pH of a solution of 0.300 M HNO, containing 0.180 M NANO,? (Ka of HNO2 is 4.5 x 10-4)

A: Given- Concentration of HNO2=0.300M Concentration of NaNO2=0.180M Ka of HNO2= 4.5×10-4

Q: What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.47 M in HIO? The Ka for HIO is 2.3…

A: When a weak acid(eg HIO) mixed with its conjugate base (ege IO-) they form a buffer solution. pH of…

Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

A:

Q: For the diprotic weak acid H2A, Kal = 3.9 x 10-6 and K22 = 7.7 x 109 What is the pH of a 0.0400 M…

A: The hydronium ion concentration can be calculated using ICE table as,

Q: What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium…

A: Since CH3NH2 is a weak base with pKb = 3.38 And the solution is having CH3NH2 and its conjugate acid…

Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…

A: Ka = 6.20×10-10 pKa = -log(Ka)    = -log(6.2×10-10 = 9.21  Concentration(C) of salt =0.0750 M

Q: What is the pH of a solution consisting of 0.70 M HC2H3O2 and 0.60 M NaC2H3O2 ? The Ka of HC,H3O2 is…

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: Kw = Ka x Kb  Kw = 1x10-14  given that Ka = 4x10-8 find Kb = (1x10-14) / (4x10-8) = 2.5x10-7 Initial…

Q: What is the pH of a solution that is 0.400 M in NH3 and 1.450 M NH4*? Ka= 5.7x1010

A: Given :-  Concentration of NH3 = 0.400 M  Concentration of NH4+ = 1.450 M  Ka = 5.7 × 10-10  To…

Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

A:

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given: Concentration of NaClO = 0.059 M

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

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :-  Initial concentration of weak acid = 0.17 M  Ka for acid = 2.1 × 10-5  To be calculated :-…

Q: Calculate the pH of a solution that is 0.155 M in NH3 acid and 0.255 M in NH4Cl. The Kb of ammonia…

A: Weak acid and its conjugate base forms a buffer solution similar to a weak base and its conjugate…

Q: What is the pH of a solution that is 0.75 M HF and 0.15 M NaF?   The Ka of HF is 6.6 x 10-4

A: Given: Concentration of HF [HF]= 0.75 M Concentration of NaF [NaF]= 0.15 M Ka of HF is 6.6 x 10-4 To…

Q: What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O…

A: ​Given - - - >   Ka = 3.5*10-8   pH = 0.25

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: Calculate the ph of a solution that is made by dissolving 6.45g of NH4Cl(53.49g/mol) in enough water…

A: First calculate molarity by mole/volume. Then use weak base concept to get pH

Q: NH3 is a weak base (?b=1.8×10^5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: What is the pH of a 75.0 mL solution that is 0.049 M in weak base and 0.055 M in the conjugate weak…

A: The pH can be calculated by using Henderson equation  poH =pkb +log10 [ conjugate acid]/ [weak base]

Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: The Ka of propanoic acid (C,H,COOH) is 1.34 x 10-5. Calculate the pH of the solution and the…

A:

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A:

Q: Aniline, C6H5NH2 is a weak base important in the dye industry.  It has a Kb= 4.0 x 10-10. What is…

A: Step : 1           What is the pH of a solution containing 0.45 M aniline?

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: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: What is the pH of a solution that is 0.26 M CH3NH2 (methylamine) and 0.38 M CH3NH3Cl (methylammonium…

A: The basic buffer may be explained as the solution mixture which hold the weak base along with its…

Q: Kb for ammonia (NH3) is 1.76 x 10-5     What is Ka for ammonium, its conjugate acid. (NH4+)

A:

Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?

A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…

Q: HClO 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: It is required to calculate the pH of the solution that is 0.016 M in NaClO.Ka for HClO = 4 x 10-8…

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

A:

Q: If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.19 M solution of this acid?

A: Given, Concentration of monoprotic weak acid = 0.19 M Ka of monoprotic weak acid = 8.3 × 10-6

Q: What is the pH of a solution with hydroxide concentration, [OH--] = 4.83×10-5 M?

A: According to the question,  We need to calculate the pH of a solution with hydroxide concentration,…

Q: The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5).What is the pH of a 0.258 M…

A: 1) Given: Concentration of C6H5COOK = 0.258 M The hydrolysis reaction of C6H5COO- coming from…

Q: The Ka for niacin is 1.5 x 10-5. Whatis the pH of a 0.010 M solution of niacin?

A: The dissociation reaction of niacin is as shown below Hence we can see that 1 molar concentration…

Q: What is the theoretical pH of a 0.10 M NH4Cl solution when the Kb for NH3 is 1.8 x 10^-5?

A:

Q: What is the pH of a 0.20 M solution of sodium acetate? The Ka for acetic acid is 1.8x10-5 ?

A: Given, Concentration of sodium acetate = 0.20 M Ka of acetic acid = 1.8 x 10-5 Formula used, [OH-] =…

Q: What is the pH of a solution that is 0.29 M KOCN and 0.14 M HOCN (cyanic acid)? (Ka for HOCN is…

A: Hensderson equation for the calculation of pH of a buffer solution consisting of a solution of weak…

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

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

Q: What is the pH of a solution that is 0.25 M CH3NH2 (methylamine) and 0.43 M CH3NH3Cl (methylammonium…

A: pH is the negative logarithm of hydronium ion. Henderson Hasselbalch equation for weak base: pKb…

Q: What is the pH of a 0.010 M solution of HF? The Ka for HF is 6.8 x 10^-4.

A: Given,   Concentration of HF = 0.010 M  Ka for HF is = 6.8x10-4

Q: What is the concentra

A: Weak acid does not dissociate completely for a weak acid,  equilibrium is established between…

Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…

A:

Q: If the Ka of a monoprotic weak acid is 4.7 x 10-6, what is the pH of a 0.49 M solution of this acid?…

A: Given Ka = 4.7 x 10-6 C = 0.49 M

Q: . What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Ka of HC2H3O2 = 1.8 x…

A:

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.