B: What is the pH of 0.6 M NH,Cl solution? Discuss your results. (K of NH= 1.8 x 10 NH4+ + H2O+→ H3O+ +NH3

Q: What is the pH of a 3.50 M solution of NH4CI (Ká of NH3= 1.8 x 105)?

A:

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: 1. Consider a solution of NaHA for which F = 0.050 mol L¹, K₁1 = 4.70 x 10³ and K₁2 = 1.80 x 10-10,…

A:

Q: Calculate the pH of a 0.381 M NH, solution. NH, has a Kp = 1.8 x 10-.

A: pH: The negative logarithm of H+ ion concentration is known as pH. Ammonia in water behaves as a…

Q: Would you expect Fe2+ to be the stronger Lewis acid? Explain.

A: A Lewis acid is a substance that accepts a pair of electrons.  A Lewis base is a substance that…

Q: What is the pH of a 0.0470 M solution of methylamine (CH&NH2, Kb = 4.4 x 10 4)?

A: Calculate the hydroxide ion concentration released by methylamine. OH- = KbCOH- = 4.4 × 10-4 ×0.047…

Q: The acid dissociation constant K, of acetic acid (HCH,CO,) is 1.8 x 10°. -5 Calculate the pH of a…

A: Since acetic acid is weak monoprotic acid. Hence it will dissociate partially as per the reaction…

Q: 2. Hypochlerous acid (HOCI) is a weak acid that forms when chlorine dissolves in water, and itself…

A: a. The central atom is O. It has two sigma bonds and two Lone Pair. That's why it has 4 coordination…

Q: What is the pH of a 0.0730 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A: Given :- concentration of methylamine solution  = 0.0730 M  Kb for methylamine = 4.4 × 10-4  To…

Q: What is the pH of a 0.860 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?

A: A numerical problem based on pH concept, which is to be accomplished.

Q: What is the pH of a 1.75 M solution of KX (Kb of X is 1.22 x 10°) (Please show the final result with…

A: Answer:  9.66 Weak base can't dissociate completely, it's  pOH = 1/2 (PKb - logC)

Q: Calculate the pH of a solution containing 0.1M NH,OH and 0.01M NH.CI, K = 1.76 x 10$. %3D

A: Given, [NH4OH] = 0.1 M [NH4Cl] = 0.01 M Kb = 1.76 × 10-5

Q: Calculate the pH that results from the addition of 1.50 mL of an 0.0126 M aqueous solution of H2SO4…

A: Gram equivalence of sulphuric acid = 1.50 x 0.0126 x 2…

Q: Find the pH of a 0.20 M aqueous solution of benzoic acid, for which Ka = 6.33 x 10-5

A:

Q: 4. What are the equilibrium concentrations of all species and the pH of a 0.20 M solution of HF…

A: The question is based on common ion effect.  Due to common ion effect of F- equilibrium of HF shift…

Q: What is the pH of (i) 1.0 X 103 M HBr and (ii) 1.0 X 102 M KOH?

A: We know that, pH and pOH can be expressed as the negative logarithm of hydrogen ion and hydroxide…

Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10 4)?

A:

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 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH of the solution…

Q: Calculate the pH of a solution of 0.1421 M KCH2ClCO2 if Ka = 1.400e-3 for CH2ClCO2H?

A:

Q: What is the pH of a 0.050 M triethylamine, (C2HS)3N, solution? Kb for triethylamine is 5.3 x 10-4

A: We should know that the amine us a basic Compound that will dissociate in solution to give basic…

Q: What is the pH of a 0.570 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?

A:

Q: Calculate the pH of a 0.75 mol L─3 solution of ethanoic acid at 298 K. Given Ka = 1.7 × 10─5

A: Welcome to bartleby ! We have to calculate pH .

Q: Calculate the pH of a 0.363 M NH, solution. NH, has a Kp 1.8 x 10-5. %3D pH

A:

Q: What is the pH of a 0.690 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: HNO2 ⇌ H+ + NO2- Ka = 4.5x10-4 = [H+][NO2-]/[HNO2] 4.5x10-4 = (x)(x)/0.690 - x  if we assume x is…

Q: What is the pH of a 0.300 M solution of aniline (CH NH, Kb = 4.3 x 10)?

A: The pH scale is given by the scientist Sorensen in order to express the [H3O+] ion of a solution. It…

Q: If the Kp of a weak base is 2.5 x 10-6, what is the pH of a 0.23 M solution of this base?

A: pH +  pOH = 14 For a weak base solution: [OH-] = (Kb x C)1/2 Where, C = molar concentration of weak…

Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: Determine the base ionization constant (in x 10-5) of a 0.0925 g sample of a weak base (molar mass =…

A: Given :- Mass of weak base = 0.0925 g Molar mass of weak base = 17.03 g/mol Volume of water = 100 mL…

Q: A 0.345 M of generic weak acid was prepared and has a Kb = 3.91 x 10-10. What is the pH of the weak…

A: Answer: On adding in water partial dissociation of weak acid takes place and an equilibrium is…

Q: A weak acid (IHA) has a Ka 1.0 x 10, If you test and find the [II']-0.001, what is the pH and…

A: Given: [H+ ] = 0.001 M And the Ka of HA = 1.0 × 10-5

Q: What is the pH of a 0.0360 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 10-10)?

A:

Q: 6. What is the pH of a 0.25 M solution of methylamine hydrochloride (CH3NH3CI)? Kb for methyl amine…

A: This ia a salt of weak base and strong acid. So apply formula for salt of weak base and strong acid.

Q: The Kp of dimethylamine [(CH3)2NH] is 5.90×104 at 25°C. Calculate the pH of a 1.55x103 M solution of…

A: Given :  Concentration of (CH3)2NH = 1.55 × 10-3 M  Kb = 5.90 × 10-4  To calculate :-  pH of…

Q: What is the pH of a 0.300 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: CH3NH2 is a weak base that partially dissociates in water. C6H5NH2(aq) ↔ OH-(aq) + C6H5NH3+(aq)…

Q: The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH] in the…

A:

Q: What is the pH of 0.273 M trimethylammonium iodide, (CH3)3NHI? The Kb of trimethylamine, (CH3)3N, is…

A: Kb = 6.3 x 10-5

Q: 2. What is the value of k?

A: OH- + C24H30N3+  C23H30N3-OH The general rate law is   [rate] = k [OH-]^x [ C24H30N3+]^y For the…

Q: 0.3728, 0.9319, 1.4910 and 1.8638 g aliquots of KCI were dissolved in 4 separate 250 ml samples of…

A: KCl is a salt of strong acid and strong base. As a result, it doesn't undergo hydrolysis when…

Q: Find the pH of a 0.010 M solution of morphine, another weak base with Kb = 1.6 X 10-6

A:

Q: Calculate the pH and the concentrations of all the species present in 0.010 M of Carbonic acid…

A:

Q: Alizarin yellow R, Ka = 7.9 x 1012, is yellow in its protonated form (HX) and red in its ionized…

A: Alizarin yellow (R)  be a distinct orange color when,…

Q: What is the pH of a 1.63 M solution of XOH, a weak monobasic compound (Kb = 1.7 x 10^-9)?

A: Given data in above Concentration of XOH = 1.63 M  Kb = 1.7 ×10-9

Q: What is the pH of a 0.1055 M CH3COOH solution (K, = 1.75 x 10-5)? %3D

A: Answer: ICE table for the dissociation of weak monoprotic acid is shown below:

Q: Calculate the pH of 0.0985 M CH3COOH.  MM CH3COOH : 60.05 Ka = 1.8 x 10-5

A: Given data,Molarity of CH3COOH=0.0985MMolar mass of CH3COOH=60.05g/molKa=1.8×10-5

Q: What is the pH of a 0.600 M solution of HSO, (Ka = 6.6 × 10°)? (Please show your answers with 3 sig…

A: pH of solution is equal to the negative logarithm of hydronium ion concentration. pH=-log(H3O+) Ka…

Q: What is the pH of a 0.0500 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A: Given  the base association constant, Kb = 4.4 * 10-4 Concentration of methylamine = 0.0500 M The…

Q: 4. You are given 1.500 M of HC1O,, Ką = 1.1 × 10² at 25°C. Determine its pH.

A: SOLUTION: Step 1: Since HClO2 has a low Ka value, it is a weak acid. Weak acids partially dissociate…

Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 104)?

A: Given, The pKa value of HNO2=4.5×10-4 Molarity of Ca(NO2)2= 0.680M.

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.