Q: The organic acid RCOOH has a pk = 4.08. What is the pH of a 0.50 M aqueous solution of this acid?…
A: Given: pKa of organic acid = 4.08 Concentration of organic acid = 0.50 M
Q: What is [H] in a 0.430 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 × 10 5)? %3D
A:
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: Calculate the pH of a 0.40 M solution of(C2H5)2NH (Kb=1.3x10^-3)
A:
Q: Calculation of pH (SHOW CALCULATION FROM THE GRAPH IATTACH GRAPHI 2.Find out pH at equivalent to…
A: Plot of pH vs Volume of NaOH added
Q: Calculate the pH of a 0.025 M solution of propanoic acid (Ka = 1.3 x 10-5). The answer is 1.6
A:
Q: What is the pH of a 0.260 M solution of aniline (C6HSNH2, Kb = 4.3 x 10-10)?
A: Given, MOlarity of aniline = 0.260M
Q: Calculate the pH of a 0.060 M solution of benzoic acid (C6H5CO2H) given that Ka = 6.3×10-5 for the…
A: Given: Molarity of benzoic acid is 0.060 M Ka is 6.3×10-5
Q: What is the pH of a 0.150 M solution of aniline (CeH;NH2, Kb = 4.3 × 10-1º)?
A:
Q: What is the pH of a 0.310 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)
A: Since aniline is a weak base. Hence it will dissociate as C₆H₅NH₂ (aq) + H2O (l) ------->…
Q: Calculate the pH of a 0.55 M weak base solution at 25°C. Kb = 9.1 x 10-5
A: Given : Weak base concentration = 0.55 M And Kb of weak base = 9.1 X 10-5 Assuming that the weak…
Q: Find the pH of a 0.350 Maqueous benzoic acid solution. For benzoic acid, K, = 6.5 x 10-5. a) 4.64 b)…
A: The dissociation of benzoic acid is as follows: C6H5COOHaq ↔ H+aq+ C6H5COO-I 0.350…
Q: What is the pH of a 0.290 M solution of aniline (C6H5NH2, Kb = 4.3 x 10-10)?
A: In the given question we have to calculate the pH of Aniline. concentration of Aniline = 0.290 M Kb…
Q: As2. .. What is the minimum pH needed to prepare 1% sodium phenobarbital in water? Intrinsic…
A: We have to prepare 1% sodium phenobarbital in water. Solubility = 0.004M MW = 232.2g/mol pKa = 7.41
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: 9. If only 0.9% of 0.50 M solution of a weak base was ionized. Calculate its Kb value? * 1.6 x 104…
A:
Q: What is the pH of 1.10 M CrCl3 (K = 1.00x10-4)? %3D
A: Given, Concentration of CrCl3 (C) = 1.10 M Ka = 1.00 × 10-4 pH of the solution = ? Note: pKw = 14…
Q: What is the pH of a 0.03 M solution of sodium benzoate (C6H5COONa)? Ka = 6.6 *10-5.
A: It is given that 0.03 M sodium benzoate (C6H5COONa) is present, and the equation is written as…
Q: B: What is the pH of 0.6 M NHẠC1 solution? Discuss your results. (Kb of NH= 1.8 x 105) NH4* + H2O+…
A: In the given question we have to calculate the pH of 0.6 M NH4Cl Solution. we know that the ammonium…
Q: What is the pH of a 0.36 M solution of HNO2 (Ka = 4.5 x 10-4)?
A:
Q: Calculate the pH of a 0.025 M solution of propanoic acid (K, = 1.3 x 10-5). 7.48 0.025 O 5.6 x 104…
A:
Q: Calculate the pH of a 0.0153 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4)
A:
Q: Calculate the pH of a 0.60 M solution of ethylamine(C2H5NH2, Kb = 5.6 x 10-4.)
A:
Q: 6. What is the pH of 0.5 M nitrous acid (HNO2) ( Ka = 4.5 x 10-4) %3D www
A: Find the pH of HNO2 having 0.5 molarity Given ka = 4.5 x 10-4
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: Calculate the pH of 0.045 C5H5N (Pyridine) K_b= 1.7 x 10^-9 for C5H5N
A: We will ionize pyridine , then draw ICE table to calculate pH of solution.
Q: The Kb for ethylamine (C2H5NH2) is 5.6 x 10-4. What is the pH of a 0.020 M solution of ethaylamine?
A: The reaction is – C2H5NH2 + H2O↔C2H5NH3+ + OH-I 0.02…
Q: What is the pH of a solution that is 0.048 M in HA and also 0.042 M in NaA? (Ka = 4.1 x 10-6) 6.82…
A: Given, Ka for NaA = 4.1 x 10-6 PH = ?
Q: What is the pH of a solution with a fluoride concentration of 0.20 M ? The Kb for F– is 1.47×10-11 .
A: In order to find the pH of the solution we first write down the given data: Fluoride concentration=…
Q: The pH for 0.050 M CH3NH2 (Kb for CH3NH2 = 4.0 X 10^-4 )?
A:
Q: Calculate the pH and percent ionization of 0.05 M acetic acid Ka = 1.8 x 10 -5. %3D
A: Given, Concentration of acetic Acid (C) = 0.05 M Ka for acetic acid = 1.8 × 10-5 pH = ? Percent…
Q: What is the pH of a 0.64 M solution of NH3 (Kb = 1.2 × 10-5)?
A:
Q: B: What is the pH of 0.6 M NHẠC1 solution? Discuss your results. (Kp of NH= 1.8 x 105)
A: formula p H = 7 - 1/2 [PKb + logc]
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: What is the pH of a 0.0670 M solution of methylamine (CH3NH2, Kb = 4.4 x 104)? %3D
A:
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: Find the pH of a 0.600 M solution of methylamine CH3NH2. Kb = 4.4 x 10-4. %3D
A: Given,Concentration of methylamine = 0.600M.Kb = 4.4*10-4.
Q: Calculate the pH of a 0.20 M solution of NH4NO3 Kb(NH3) = 1.8x10^-5 Thank you :)
A: A pH scale is a scale that is used to determine the acidic and basic nature of a solution. If the pH…
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 Ka for the conjugate acid of C₅H₅N (Kb = 1.7 × 10⁻⁹)?
A: Kw is ionization constant for water . Ka and kB ionization constant for Acid and base respectively…
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: 11. Calculate [H3O*] for a solution of pH = 4.987. %3D
A: The relation between pH and [H3O+] is: From pH, get [H3O+] by rearranging the equation:
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: Find the pH of a 2.5 M solution of KCLO2 ( HCLO2 Ka= 1.1 x 10^-2)
A: Given Molarity of KClO2 = 2.5 M Ka (HClO2 ) = 1.1 * 10-2pKa = -log KapKa = -log 1.1 * 10-2pKa…
Q: Find the [H2L*] concentration in a 0.005 M leucine hydrochloride aqueous solution (H2L*). H2L, Ka, =…
A:
Q: 9 what is the PH of a 2.5 M solutien ef CH, NH, CI ? CHgNHz pkb = 3.35) %3D
A:
Q: Find the pH of a 0.204 M KClO solution. (The Ka of hypochlorous acid, HClO is 2.9×10-8
A: Kclo is a salt of weak acid and strong base so use the formula of PH of salt. PH=10.4
Q: Ex 2) Acids and Bases: A solution is obtained by completely dissolving 900 g of sodium hypochlorite…
A: Answer:- This question is answered by using the simple concept of calculation of pH of solution…
Q: What is the pH of a 0.35 M solution of methylamine (CH3NH2, Kb 4.4 at 25°C? O a. 5.55 b. 12.09 O c.…
A: We will. Calculate pH
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- What is the Ph of a 0.23 M triethylamine (C2H5)3N solution? Kb for triethylamine is 5.3 x 10^-4. Report 2 decimal places.Wgat is the [OH-] of a bleach sample that registers 11.41 on a pH meter?2,What is the pH of the solution with hydronium ion concentration of 6.3 x 10-12 M? Group of answer choices 10.80 12.60 11.20 11.80 10.20 3,Calculate the pH of 0.50 L of the solution containing 5.61.0g KOH dissolved at 25oC. Group of answer choices 13.30 13.00 0.33 13.70 1.33 4. Calculate the [H3O+]of the solution with pH=9.2. Group of answer choices 2.0 x 10-10 3.6 x 10-9 6.3 x 10-10 9.2 x 10-9 2.0 x 10-9
- Im doing a lab report on the creation of soap through the saponification process, and am currently figuring out a second source of error to include. The ph value of the soap I created is ph8. According to multiple websites, the normal ph value for homemade soaps is around 9-10. What source of error woudlve caused the ph of my soap to be lower?Find the value of Kb given a 50.0 mL solution of 5.03x10-2 M (CH3)3N, with a pH of 11.25 at 25ºC. (CH3)3N + H2O↔ (CH3)3NH+ + OH- a. 6.52x10-5 b. 1.53x10-10 c. 6.73x10-10 d. 1.78x10-5The pKa of an HA acid is 6.00. What would be the pH (to 2 decimal places) of a solution initially containing HA 0.100 mol L-1, NaA 0.100 mol L-1 and HCl 0.020 mol L-1?
- pH calculation when the second equivalence pointis reached: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 50.0 ml of 0.500 MNaOH. Round your calculated value for pH to twofigures to the right of the decimal point. Significantconstants: Ka1 of oxalic acid = 5.60 x 10^-2 and Ka2of oxalic acid = 5.42 x 10^-5How many milliliters of 0.500 M NaOH should be added to 100 mL of solution containing 3.0 g of L-lysine dihydrochloride (formula mass = 219.11 g/mol) to get a pH of 9.27? (Provide a numerical response only.) pka1=1.77, pka2=9.07In a preparation, a 0.5% epinephrine HCl (E = 0.29) with sterile water qs to make 30 ml, with ph of 5.0. how many grams of epinephrine is needed? and the ml of h2O needed to make the preparation isotonic?
- Suppose a biochemist has 10 mL of a 1.0 M solution of a compound with two ionizable groups at a pH of 7.50. She adds 10.0 mL of 1.0 M HCl, which changes the pH to 3.80. The p?a value of one of the groups is p?1=4.10 and it is known that p?2 is between 7 and 10. What is the exact value of p?2? Enter your answer to two significant figures. p?2 = ??Calculate the pH after addition of 24.12 mL of 0.1021 M HI to 25.00 mL of 0.1698 M CH3CH2CH2NH2. Kb(CH3CH2CH2NH2) = 5.100e-4.A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 × 10–6 and Ka2 = 1.0 × 10–10) is titrated with 2.00 M NaOH. How many mL of 2.00 M NaOH must be added to reach a pH of 12? Give answer in 15 min.