HCIO is a weak acid (K₁ = 4.0 × 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a solution that is 0.064 M in NaCIO at 25 °C? pH =

Q: What is the pH of a solution that is 0.200 M ammonia (NH3) and 0.150 M ammonium chloride (NH4Cl)?…

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Q: A solution is prepared at 25 °C that is initially 0.057M in dimethylamine ((CH, NH) a weak base with…

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Q: the solutions are additive and that Kp = 4.4 x 104 for methylamine.

A: The question is based on the concept of EQUILIBRIUM. we have to calculate pH of the solution…

Q: A solution is prepared at 25 °C that is initially 0.45M in methylamine (CH,NH,), a weak base with…

A: Solution- Here we have basic buffer with Kb ; basic ;  CH3NH2=0.45 M Acid; CH3NH3Br = 0.49M Kb= 4.4…

Q: The lonization constant, K₂. for HCN(aq) is 6.2 x 10-10. What is the pH of a 0.10 molar solution of…

A: Given Concentration = 0.10 M Ka = 6.2 * 10-10

Q: The Kb for methylalmine, CH3NH2, is 4.47 x 10-4. What is the pH of a 0.250 M solution of CH3NH2?

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Q: Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the…

A: The dissociation of tartaric acid can be represented as: H2C4H4O6+H2O↔HC4H4O6-+H3O+…

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

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Q: Calculate the pH of a 0.10 mol L-1 solution of barium hydroxide, Ba(OH)2.

A: Given, concentration of barium hydroxide = 0.10 mol/Lwe know that barium hydroxide is a strong base…

Q: H3 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: 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: Given: Kb = 1.8 × 10-5              Concentration of solution = 0.056 M             Temperature = 25…

Q: A solution is prepared that is initially 0.0010 M NaOH and 0.10 M NH3. What is the pH of this…

A: [NaOH] =0.001 M [NH3] = 0.10M

Q: What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization…

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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: NH3 is a weak base (K, = 1.8 × 10-5) and so the salt NHCI acts as a weak acid. What is the pH of a…

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

A: The ionization of NH4Cl as follows,

Q: The temperature for each solution is carried out at approximately 297 K where K w =1.00×10 −14 0.85…

A: Given, Kw = 1.00*10-14. Mass of HCl = 0.85g. Volume of solution = 5.5L. Moles and molarity of HCl…

Q: At 50°C and 1 atm, K(w)=5.19X10⁻¹⁴. At these conditions,find (a) [H₃O⁺] in pure water, (b)…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

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:

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

A: Given-> Concentration of KCN = 0.0795 M Ka(HCN) = 6.20 × 10-10

Q: A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 moles of sodium…

A: The ratio of the number of moles of a solute dissolved per litre of solution is called the…

Q: 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…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

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Q: A solution of acids is made by mixing 0.19 M HNO3 and 0.45 M CH3COOH (Ka (CH3COOH) = 1.8 x 10-5).…

A: To calculate the pH of the solution, we need to consider the acid dissociation reactions of both…

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: A solution is prepared that is initially 0.49M in pyridine (C5H₂N), a weak base, and 0.40M in…

A: Given: The concentration of pyridine = 0.49 M The concentration of pyridine chloride = 0.40 M…

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 made from combining 2.49 mol (CH3)2NH2Cl and 5.18 mol (CH3)2NH in a…

A: Henderson-Hasselbalch equation explains the relationship between  of solution and  of acid. For a…

Q: NH3 is a weak base (K₁ = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: NH4Cl is a salt of weak base NH3 and strong acid HCl. So in an aqueous solution of the salt the salt…

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

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

A:

Q: What is the pH of a 0.0801 M solution of this acid?

A: Given :-  Initial concentration of acid = 0.0801 M  Ka = 2.43 × 10-5   To calculate :-  pH of the…

Q: HClO is a weak acid (?a=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Given : Concentration of NaClO = 0.014 M Since NaClO is a weak conjugate base of weak acid HClO.…

Q: Consider a 1.0 L of 0.1 M aqueous solution consisting of weak acid HA, which has K₂ = 3.9 x 10-4, at…

A: HA is a weak acid that is very weakly dissociated to give H+(aq) ions. HCl is a very strong acid…

Q: What is the pH of 1.000 L of a solution of 100.0 g of glutamic acid (C5H9NO4, a diprotic acid; K1 =…

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Q: Calculate the magnitude of the equilibrium constant for benzoic acid, HC7H5O2, if a 0.100 M solution…

A: The benzoic acid represented as C6H5COOH. It is a weak acid and dissociate into hydrogen and…

Q: HClO is a weak acid ( ?a=4.0×10^−8 ) and so the salt NaClO acts as a weak base. What is the pH of a…

A: pH of a solution of a salt of weak acid and strong base:pH = 7 + (pKa + logC)/2

Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10,…

A: a) Given: Volume of HF=50 mL Concentration of HF= 0.2 M Concentration of NaH2BO3= 0.5 M Volume of…

Q: The K, of a weak monoprotic acid is 1.65 x 10-5. What is the pH of a 0.0859 M solution of this acid?…

A: In this question, we want to determine the pH of the weak monoprotic acid,  How we can determine the…

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.