Calculate the pH value of a 0.20 M solution of NH4Cl (Kb (NH3)= 1.79 × 10 -5).

Q: A solution is prepared at 25 °C that is initially 0.25M in methylamine (CH,NH,), a weak base with…

A:

Q: Calculate the pH of a solution (aq., 25 oC) prepared by dissolving 48.026 g of ammonium nitrate (mm…

A: In this question, we want to determine the pH of a solution.  You can see details Solution below…

Q: Determine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given…

A: Given,  The molarity of each solution in 1 L beaker is 0.035 M.  The pH of the solution is:

Q: What is the pH of a 0.250 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Given data,Molarity of aniline=0.250MKb=4.3×10-10

Q: The base protonation constant K, of lidocaine (CH, NONH) is 1.15 × 10 °. 8- 14 Calculate the pH of a…

A: Lidocaine being a weak base , dissociates partially in water. The dissociation is lidocaine in water…

Q: What is the pH of a solution that is 0.14 M C,H, NH2 (ethylamine) and 0.51 M C;H;NH;Br…

A: Given :  Here ethylamine is acid while ethylammonium bromide is salt. So, [Acid] = 0.14 M And [Base]…

Q: Calculate the pH of a 1.16 M aqueous solution of pyridine hydrochloride (C5H5NHCl). (For pyridine,…

A: Given :

Q: Calculate the ph of 0.24m sr(oh)2 aq 0.05m nh3 (kb=1.8*20^-5)

A:

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: A solution is prepared at 25 °C that is initially 0.32M in diethylamine a weak base with K,= 1.3 ×…

A: Below attached file showing the details answer. All the best.

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

A:

Q: The base protonation constant K, of allantoin (C,H,N,0,NH,) is 9.12 x 10 °. Calculate the pH of a…

A: Given-> Kb of allantoin = 9.12 × 10-6 Molarity = 1.3 M

Q: Calculate the pH of a 4.80×10-1 M aqueous solution of sodium nitrite (NaNO2). (For nitrous acid,…

A:

Q: The acid dissociation Ka of acetic acid HCH3CO2 is ×1.810−5. Calculate the pH of a ×6.610−1M aqueous…

A: The dissociation of acetic acid can be given as

Q: What is the pH of a 0.220 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Aniline is a weak base.  C6H5NH2+H2O⇔C6H5NH3++OH-      1                                  0…

Q: Calculate the pH of a solution of 0.15 M C5H5N. (Kb = 1.7 x 10^-9)

A: It is weak base so we will use concept of weak base.

Q: Calculate the pH of a 0.210 M solution of sodium benzoate

A: Benzoate is the conjugate base of benzoic acid. In water, benzoate hydrolyses as follows...…

Q: Calculate the pH at 25]°C of a 0.14 M solution of a weak base with a Kb of 3.8 ×10−11.

A: Considering the dissociation of a weak base,

Q: Determine the pH of solution if 0.085g of acetylsalicylic acid, HC9H7O4, (Ka = 3.0 x 10-5) is…

A:

Q: Calculate the pH of a 0.100 M solution of a weak base, A-, given Kb = 6.38×10-6.

A:

Q: What molar concentration of hydrazine, N2H4 (Kb = 1.7 x 10^-6) yields a solution with a pH of10.46?

A: The objective of this question is to find the molar concentration of hydrazine, N2H4 that yields a…

Q: Calculate the pH of a 0.0269 M aqueous solution of the weak base piperidine (C5H1₁₁N, K₁ =…

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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…

A:

Q: What is the pH of a 0.290 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Find PH using ICE table and some farmula

Q: Find the pH of a 0.200 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C.

A:

Q: what is the ph of a 0.85 M solution of pyridine (C5H5N, Kb = 1.70 x 10 ^-9)

A: Pyridine is a weak base. pOH of a weak base. pOH = -log [OH-] pH = 14 - pOH For a weak base like…

Q: A solution is prepared at 25 °C that is initially 0.44M in ammonia (NH3), a weak base with K₂= 1.8 ×…

A: Solution that  contains weak base (ammonia) and corresponding salt (ammonium chloride) of strong…

Q: Calculate the pH of a 0.431 M aqueous solution of acetylsalicylic acid (aspirin) (HC,H,0, K, =…

A: given concentration of acetylsalicylic acid = 0.431M Ka = 3×10-4

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

A: Kb = 1.8 × 10-5Concentration of NH4Cl = 0.025M Temperature,T = 25°CpH of the solution=?

Q: Calculate the pH of a 0.321 M aqueous solution of hydrofluoric acid (HF, K₂ = 7.2x10-4). pH =

A: we have to calculate the pH of solution

Q: Calculate the pH of an aqueous solution that is ( Ka(HCN) = 6.20 × 10 10-10) a. 0.870 M in HCN. pH =…

A: We know that  HCN is a weak acid it doesn't dissociate completely. The dissociation reaction will be…

Q: Calculate the pH of a 6.00×10-1 M aqueous solution of hydroxylamine hydrochloride (HONH3Cl). (For…

A: The question is based on the concept of salt hydrolysis. we have to calculate pH of given…

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: 0.21 M CH3NH3I (Kp (CH3NH2) = 4.4 × 10-4)

A: Given data: Dissociation constant of base (Kb) = 4.4 x 10-4  Concentration of CH3NH3I = 0.21 M…

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe.  Out…

A: Given,  0.050 M in H2Se 0.075 M in NaHSe

Q: Calculate the pH of a 0.22 M codeine solution (Kb = 1.6ã10−6).

A: The value of Kb for the given weak base is = 1.6x10-6 The concentration of the base solution is =…

Q: Ka(HCN) = 6.2 x 10-10. Determine the pH of 0.82 M NaCN aqueous solution (3 significant figures).

A:

Q: The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydrox concentration and the…

A: The dissociation of ammonia in aqueous solution can be represented as: The ionization constant for…

Q: What is the pH of a solution prepared by adding 18.0 mL of 1.51 M nitric acid to 180.0 mL of 0.150 M…

A:

Q: What is the pH of a 0.130 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A:

Q: Calculate the pH of 0.606 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for…

A: pH of C6H5NH3Cl = to be calculated  Concentration of aniliniun hydrochloride = 0.606M Kb for aniline…

Q: Calculate the pH of 0.750 M pyridinium chloride, C5H5NHCl? Given Kb of C5H5N is 1.70×10-9.

A:

Q: A solution is prepared at 25 °C that is initially 0.48M in diethylamine (C,Hs) NH), a weak base with…

A:

Q: The pH for 0.050 M CH3NH2 (Kb for CH3NH2 = 4.0 X 10^-4 )?

A:

Q: 0.185 M in HCHO2 (Ka = 1.8 × 10-4) and 0.230 M in HC2H3O2 (Ka = 1.8 × 10¬5) Express your answer to…

A: Answer: In this question we have to find out the pH of the solution of two weak acids. In the…

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

A: Handerson Hasselbalch equation –  Buffer solution is mixture of weak acid and its conjugate base.…

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.