Q: Which is a stronger acid, H2O or H2S?
A: According to Arrhenius theory an acid is the substance which gives H+ ions when dissolved in water.…
Q: Calculate the pH of a 1.22×10-2 M solution of the decongestant ephedrine hydrochloride if the pKb of…
A: The pH of the decongestant ephedrine hydrochloride can be calculated as
Q: What is the pH of a 0.360 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹
A: Given data--> C= 0.360 M solution of C5H5NHBr Kb=1.7*10-9 pkb = - log10(1.7*10-9) pkb= 9 -…
Q: What is the pH of a 0.710 M solution of C5H5NHB (Kb of C5H5N is 1.7 x 10-9)?
A: pH is used to determine the concentration of hydronium ion.
Q: The base B has pKb 5.00. (a) What is the value of pKa for the acid BH? (b) At what pH is [BH] …
A: Handerson Hasselbalch equation – Buffer solution is mixture of weak acid and its conjugate base.…
Q: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0341 M methylamine (CH3NH2)…
A: The given data contains, Concentration of methylamine = 0.0341 M. Kb of CH3NH2 is 4.47×10−4.
Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A:
Q: Consider two acids: C,H5CO,H (benzoic acid, pK = 4.2) and HCO,H (formic acid, pK=3.8). Which acid is…
A: We are having two acids benzoic acid and formic acid we have to choose the strongest acid .
Q: Relative Acid Strength 2.51 Rank the following compounds in order of increasing acidity он NH2 HO,…
A: Since you have posted multiple independent questions in the same request, we will solve the first…
Q: What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)
A: Given, Concentration of C₅H₅NHBr = 0.420 M Kb = C₅H₅N is 1.7 × 10⁻⁹ pKb=-[logkb]pKb=-[log 1.7 ×…
Q: What is the pH of a 0.650 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A:
Q: Calculate the pH of a 0.0015 M solution of C6H5NH2 (Kb for C6H5NH2= 3.80 x %3D
A: given :- concentration of C6H5NH2 = 0.0015 M Kb for C6H5NH2 = 3.80 × 10-10 To calculate :- pH of…
Q: What of the following options describes the term "strong acid/base"? O a. A pair of species which…
A: A strong acid or strong base is a strong electrolyte.
Q: What are the concentrations of H3O+ and OH− in oranges that have a pH of 3.71?
A: pH :- The negative logarithm to the base 10 of hydronium ion concentration expressed in mol/L of…
Q: The base protonation constant K, of azetidine (C,H,NH) is 1.5 × 10 °. Calculate the pH of a 0.44 M…
A:
Q: Calculate the PH of4.6M formic acid (CHOOH) solution given a ka value of 1.787*10^-4
A:
Q: What is the pH of a 1.47 mol/L solution of HCN(aq) if its Ka = 3.5 ´ 10-11?
A: HCN is a weak acid hence it can dissociate partially Ka value of HCN=3.5×10^-11
Q: Calculate the pH and [S2−] in a 0.10-M H2S solution. Assume ka1= 1.0 × 10−7; ka2= 1.0 × 10−19.
A: Answer:- This question is answered by using the simple concept of calculation of pH of a weak acid…
Q: Calculate the AH for the reaction (6 points)
A: Calculate the ∆H for the reaction., NO(g) + O(g) → NO₂(g)
Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A: Given information: Concentration of solution = 0.510 M
Q: If the Ka of the conjugate acid is 7.68 × 10-4 , what is the pKb for the base?
A: Applying relationship between ka and kb Ka× kb= Kw
Q: ∠AGH and ∠ DHE are
A: It seems that this is the angle of any geometrical figure .
Q: Calculate the pH at 25°C of a 0.64M solution of anilinium chloride C6H5NH3Cl. Note that aniline…
A: The pKb of C6H5NH2 is 4.87. The pKa of C6H5NH3+ is calculated using equation (1).
Q: What is the pH of a 0.650 M solution of C5H;NHB (Kb of CsH;N is 1.7 × 10-º)?
A:
Q: A weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?
A: Given pH = 3.7 Initial Concentration = 0.020 M
Q: -NH2 но NH b. OH
A:
Q: If the Ka of the conjugate acid is 2.78 × 10-7 , what is the pKb for the base
A: Based on Bronsted theory, whenever a base accepts a proton that is H+, the formation of conjugate…
Q: What is the pH of a 0.430 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A: pH= 1/2(pKb-logc) Here given Kb=1.7×10-9,hence pKb=-logKb=-log(1.7×10-9) given c=0.430 M
Q: Calculate the pH of a 0.0200 M solution of ibuprofen (isobutylphenylpropionic acid, C,2H17COOH)…
A:
Q: Consider two acids: Cl,CHCO,H (dichloroacetic acid, pK,=1.3) and HCO,H (formic acid, pK, = 3.8).…
A: In this question, we will select the strongest acid. You can see details explanation and answer…
Q: What is the pH of a 0.380 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A:
Q: What is the predominant form of ammonia in a solution at pH 7.0? Approximately what fraction is in…
A: pH of compound is the negative logarithm of its hydrogen ion concentration. The pH of a compound…
Q: Estimate the pH of 0.0025 M NH(CH3)3Cl(aq) at 25°C. It is given that trimethylamine ((CH3)3N) has a…
A: Given : Concentration of salt = 0.0025M pKb = 4.19
Q: Calculate the formate ion concentration and pH of a solution that is 0.050 M in formic acid %3D
A: Given data : Molar concentraion of Formic Acid = 0.050 M . Molar concentraion of Nitric Acid =…
Q: The pH for 0.050 M of CH3NH3Cl ?
A: Methylammonium chloride (CH3NH3Cl) dissociates into quaternary ammonium ion (CH3NH3+) and chloride…
Q: What is the pH of a 0.639 M solution of lactic acid? The pKa of lactic acid is 3.854.
A:
Q: Consider two acids: CH;CO,H (benzoic acid, pK, = 4.2) and CH,CO,H (acetic acid, pK,= 4.8). Which…
A: According to Bronsted-Lowry concept Acid is a substance which donates proton to other and forms its…
Q: A 2.5 M solution of formic acid (HCOOH) has a pH of 1.67. What is the pK, of the formate ion…
A: Welcome to bartleby ! We have to calculate pKb
Q: (е) Ва(NO,),(аq) + NaOH(aq)-
A:
Q: What is the pH of a 0.500 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A:
Q: If the Ka of the conjugate acid is 4.39 × 10-8 , what is the pKb for the base?
A: Acid dissociation constant (Ka) and base protonation constant (Kb) can be mathematically expressed…
Q: Calculate the pH at 25°C of a 0.91 M solution of anilinium chloride (C6H5NH3Cl). Note that aniline…
A:
Q: Consider the weak base ammonia. a) Write a balanced net ionic equation for aqueous solutions of…
A: Equilibrium constant in terms of concentration is the ratio of the concentration of product to the…
Q: 665 mL of 0.875 M aque ous aniline solution CC2H5 NH) are boiled gently to reduce the volume to 401…
A: Calculation of final molarity of aniline after boiling: M1V1=M2V20.875 M×665 mL=M2×401 mLM2=1.451 M
Q: The pH for 0.0850 M solution of C6H5CH2COOH is 2.68. Determine the value of Ka for C6H5CH2COOH.
A: Given pH of C6H5CH2COOH is = 2.68. We Know, pH = - log[H3O+] So, 2.68 = - log[H3O+] Or, log[H3O+] =…
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- 4. A student has prepared 0.05 M solution of CH3-C=CH and has added to it 0.05 M solution of potassium tert-butoxide (K" O-C(CH3)3). (i) Write the equation for the acid-base reaction that might occur. (ii) With curved arrows track the movements of electron pairs. (iii) Assign Base, Acid, Conjugate acid for the base, Conjugate base for the acid. (iv) Calculate the percentage of deprotonated methyl acetylene taking into account that pKa of the conjugate acid of potassium tert-butoxide equals 18 and pKa of methyl acetylene equals 24.3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.3. For the following acid - base reaction, (a) predict the products; (b) identify the Bronsted acid, Bronsted base, conjugate acid, and conjugate base; (c) use curved arrows to show the flow of electron pairs in the reaction. CH3 CH2C-OH + NaNHa
- For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36(4) Define Lewis acid/base versus Bronsted acid/base and describe the other two effects that influence acidity (hybridization and resonance)(47) (244) (243 Nonmetal Which is the strongest acid of the following? O HIO O HBRO HOAT O HCIO O HCIO2 Previous