Q: Calculate the pH of 0.50 M sodium acetate, CH3COONa. Ka(CH3COOH) = 1.8 x 10-5 5.72 11.48 2.52…
A: Given;
Q: What is the pH of a 3.50 M solution of NH4CI (Ká of NH3= 1.8 x 105)?
A:
Q: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10¯11. What is the pH…
A: The Ka1 is greater than Ka2 by a fraction of 10-4. In a diprotic acid, firstly the first hydrogen…
Q: Calculate the pH of a 0.40 M solution of(C2H5)2NH (Kb=1.3x10^-3)
A:
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: 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: Calculate the pH of 0.2 M HNO2 solution (ka=4.5*10-5)
A: we know PH=-logH+HA⇆H++A- (acid)So, Ka=H+A-HA
Q: Calculate the pH at 25°C of a 0.45 M aqueous solution of oxalic acid (H2C2O4). (Ka1 and Ka2 for…
A: We have to calculate the pH value.
Q: 11.) Calculate the pH of the following solutions: a.) 0.100 M solution of HNO2 (Ka = 4.5 x 10–4)…
A: (11a)
Q: What is the pH of a solution of 0.300 M HNO2 containing 0.210 M NANO2? (Ka of HNO2 is 4.5 x 10-4)
A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…
Q: The pH of a solution that is 0.5 in MA and 0.3 in HA is 5.40; determine the pKa of the acid.
A:
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: Calculate the pH of a 0.4 M pyridine solution, Kb=2.0x10-9
A: The value of Kb for the given weak base is = 2.0x10-9 The concentration of the base solution is =…
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: What is the pH of a solution of 0.300 M HNO₂ containing 0.170 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
A: pH of a solution is defined as the negative logarithm of H3O+ ion concentration. Here the given…
Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)?
A: Given concentration of CH3COOH = 1.75 × 10-5
Q: What is the pH of a 0.0600 M solution of nitrous acid at 25 C?
A: Since nitrous acid is a weak acid with acid dissociation constant = 5.6 X 10-4 The dissociation…
Q: Calculate the pH of a 0.125 M sodium propionate (NaC3H5O2) solution
A:
Q: What is the pH of 0.41 M HCIO? Ka = 3.0 x 10-8? %3D
A: We are provided with information, [HClO] = 0.41 M Acid dissociation constant Ka = 3.0 × 10-8 We…
Q: Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed…
A:
Q: What is the pH of an aqueous solution that is 0.011 M CH3COOH (Ka = 1.8 x 10-5) and 0.019 M…
A: An aqueous solution containing weak acid (CH3COOH) and it's conjugate base (CH3COONa) results in the…
Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.140 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
A: Given : Concentration of HNO2 = 0.300 M Concentration of NaNO2 = 0.140 M And Ka of HNO2 = 4.5 X 10-4…
Q: Calculate the pH of a 0.350M aqueous solution of NH3 , The Kb of NH3 is 1.77 x 10-5
A: Given: The concentration of aqueous NH3=0.350M
Q: What is the pH of a solution that is 0.033 M in HA and also 0.23 Min NaA? (Kg = 4.1 × 10-6) %3D O…
A: We have to calculate the pH of solution.
Q: What is the pH of a 0.47 M weak base solution (Kb = 9.55 x10-5)?
A: Given information: concentration of weak base solution is 0.47 M Kb = 9.55 x10-5
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: for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. calculate the ph of a 0.321 molar solution of…
A: Given, for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. The ph of a 0.321 molar solution of…
Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?
A:
Q: Oxalic acid is a diprotic acid with ionization constants Ka = 5.62 x 10- and K = 5.42 x 10-5.…
A: Potassium hydrogen oxalate is potassium salt of oxalic acid. It have second H+ ion to donate. So to…
Q: Calculate the pH for a 10.0 M solution of NH3 (kp= 1.8x105) NH3 - NH4 + OH a 13.987 O b .013 O c…
A:
Q: Determine the pH of a 0.0525M Fe(NO3)3 solution. Ka of Fe3+ = 6.3x10-3
A: Reaction of ferric nitrate in water is given below Fe3+ is formed from Fe(NO3)3.
Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.
A: Concentration of Al ion = 0.064 M
Q: What is the pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…
A: Given, The pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…
Q: 3. Calculate the pH of a 0.400 M KC2H3O2 (Ka for HC2H3O2 is 1.8 x 10-5)
A: In this question we have to tell the PH of the solution.
Q: The acid dissociation reaction for the weak acid butyric acid, HC4H¬O2 is given below. Its Ka is…
A: The dissociation reaction given is Assuming y concentration of HC4H7O2 dissociates as per the…
Q: 6. What is the pH of a solution containing 0.550 M HOAc and 0.460 M LiOAc? (ka of HOAc = 1.80 x…
A: The Henderson-Hasselbalch equation shows how the concentrations of an acid and its conjugate base…
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: Phenoxide ion (C,HsO) is a weak base, with Kp = 7.70 x 10. Calculate the pH of a 0.50 M aqueous…
A: Given that Kb = 7.70 × 10-5 Peroxide ion is a weak base
Q: What is the pH of a 0.379 M solutiôn of roxyla a. 0.42 b. 5.96 с. 3.19 O d. 6.38 O e. 4.2 x 10-7
A: Given, Molarity = 0.379 M Ka = 1.1 x 10-6 PH= ?
Q: f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A…
A:
Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 × 10-5) O 4.94 O 12.03 O 1 1.05 O 8.02 O 2.09
A: Given, Concentration of NH3 = [NH3] = 0.075 M Base dissociation constant of NH3 = Kb = 1.75 x 10-5…
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 a 0.500 M aqueous solution of HCOOH. ka = 1.77 x 10-4
A: HCOOH is a weak acid which undergoes partial dissociation in aqueous condition with degree of…
Q: What is the pH of a 0.500 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?
A:
Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.210 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
A: BUFFER SOLUTION It is a solution of weak acid or base with their corresponding conjugate base or…
Q: Calculate the pH of a solution that is 0.250 M in HClO4 and 0.125 M in CH3COOH (Ka = 1.8 x 10-5)
A:
Q: Calculate the pH of 0.0154 M NaN3. (Ka of HN3 = 1.9 x 10-5)
A: NaN3 is a salt of weak acid (HN3) and strong base (NaOH). We know, the pH of salt, which is formed…
Q: Calculate the pH of 0.0470 M LiBrO. Ka of HBrO = 2.8 x 10-9
A: The molarity of LiBrO solution is = 0.0470 M The dissociation constant of the weak acid HBrO is =…
Q: Calculate the pH of a 0.88M CH3NH2 given Kb= 4.2x10^-4
A:
Q: Find the pH and the percent hydrolysis of a 0.816 M solution of sodium o-phthalate (the salt of a…
A:
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- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)Calculate the pH of an aqueous solution containing the following: a) 0.80 M lactic acid and 0.40 M lactate ion (Ka of lactic acid = 1.38 x 10-4 b) 0.30 M NH3 and 1.50 M NH4+ (Kb of NH3 = 1.8 x 10-5)An organic acid (HA) has a molecular weight of 100. g mol-1, a Kow = 5.6 and a K, = 2.7 x 10-2. If originally 2.0 g of the acid is dissolved in 100 mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100 mL of water, what will be the pH of the water? (Consider the equilibrium processes to be sequential and unrelated chemically) O 1.89 1.48 O 2.01 1.74 O 1.61
- 1a) Determine the pH of 0.035 M NaF (pKa = 3.1). 1b) Determine the pH of 0.055 M oxalic acid (H2C2O4; Ka1 = 5.6x10-2; Ka2 = 5.4x10-5).7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid. 8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)(a) Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoic acid (C6H5COOH, Ka = 6.3 * 10-5). (b) Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.
- In which of the following aqueous solutions does the weak acid exhibit the lowest percentage ionization? (Hint: no need for calculations) * 0.01 M HC2H302 (Ka = 1.8 x 10-5) 0.01 M HNO2 (Ka = 4.5 x 10-4) O 0.01 M HF (Ka = 6.8 x 10-4) 0.01 M HCIO (Ka = 3.0 x 10-8) These will all exhibit the same percentage ionization.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95 g/mol, ka = 2.05 X 10-3) in 50.0 mL of 0.113 M NaOH and diluting the mixture to 500 mL? 1. O3.25 2. O2.04 3. O5.58 4. O6.41 5. O2.52
- The acid dissociation constants for sulfurous acid are: Ka1 3D 1.2 х 10-2 and Ka2 - 6.6 х 10-8 (a) Calculate the pH of a solution of 0.10 M H2SO3. (b) Calculate the pH of a solution of 0.10 M Na2SO3. (c) Calculate the pH of the solution resulting when equal volumes of the solutions described in parts (a) and (b) are mixed.Calculate the pH of each of the following solutions. (a) 0.109 M HONH, (Ko = 1.1 x 10-3) 4.0 9.34 X (b) 0.109 M HONH3CI 4.0 2.64 (c) pure H₂O 7.00 X (d) a mixture containing 0.109 M HONH₂ and 0.109 M HONH₂CI 4.0 6.20 XCalculate the percent ionization for bromic acid in a solution that contains 0.00850 M acetic acid and 0.200 M bromic acid. The Ka for HC2H3O2 is 1.8×10–5, and the Ka for HBrO is 2.8×10–9. THE ANSWER IS 0.00073% but I want to know how?