Q: The pH of a half-neutralized solution of a weak acid is 4.3. What is the dissociation constant (Ka)…
A:
Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.424 M ethylamine (a weak base…
A:
Q: Determine the Ka of a 0.10-M solution of hydrogen sulfate ion, HSO₄⁻, that is 1% ionized.
A: Ionisation of Hydrogen sulfate.
Q: The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous…
A: Given that, Ionisation constant of lactic acid Ka = 1.36×10-4 Amount of lactic acid dissolved in…
Q: When 0.075 mol of propionic acid, C2H5CO2H, is dissolved in 400 mL of water, the equilibrium…
A: The concentration of propionic acid and the ions has to be calculated in order to obtain the Ka.
Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.354 M diethylamine (a weak base…
A: Reaction of diethylamine with water is given below.
Q: triethanolamine
A:
Q: The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10–5. If 7.285 grams of aniline is…
A: We have to predict the equilibrium concentration of all species.
Q: Calculate the pH of the following solutions: a. 2.0 M morphine hydrochloride, C,„H,„NO,•HCI (pK, =…
A: In order to solve this question, we will be using simple concepts of chemical and ionic equilibrium.…
Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?
A: Given data,pH=2.13Molarity of HA=0.45
Q: In the laboratory, a general chemistry student measured the pH of a 0.578 M aqueous solution of…
A: For a weak acid, we have pH = 1/2(pKa - logA) where A is the concentration of the acid. Given,…
Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.421 M diethylamine (a weak base…
A: When the rate of forward reaction is equal to the rate of backward reaction then the reaction is…
Q: In the laboratory, a general chemistry student measured the pH of a 0.474 M aqueous solution of…
A:
Q: What is the pH of a 0.455 M solution of lactate, (CH3)2 COO^-1. The pKa of lactic acid, (CH3)2 COOH…
A: Given - Concentration of solution of lactate (CH3)2 COO- = 0.455 M pKa of lactic acid (CH3)2 COOH)…
Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…
A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…
Q: Dimethylamine, (CH3)2NH, a key intermediate in detergent manufacture, has a Kb of 5.9 x 10-4. What…
A: Ionic equilibrium is the equilibrium which is established between the unionized molecules and the…
Q: The hydronium ion concentration of an aqueous solution of 0.453 M hydrocyanic acid K¸= 4.00×10-10)…
A:
Q: The pH of a (1.7300x10^-1) molar solution of an aqueous weak acid (HA) is (1.99x10^0). The Ka for…
A: PHis defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…
Q: Write the expression for the acid-dissociation constant Ka for HC4H7O2. (Concentration equilibrium…
A:
Q: The acid-dissociation constants of phosphoric acid (H3PO4) at 25 degrees Celsius are Ka1 = 7.510-3,…
A: Given data contains, Molarity of aqueous phosphoric acid solution is 2.5M.…
Q: The ionization constant (Kb) of pyridine (C5H5N) is 5.62 x 10^-4. If 11.3 grams of sample of…
A: Given that - Ionization constant, Kb for pyridine = 5.62×10-4 Mass of pyridine = 11.3 grams…
Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…
A:
Q: A weak base, BOH, has a ph of 9.80 and Ka equal to 1.0 x 10-5. What is the Molarity of BOH?
A: Given data, The pOH of a weak base is calculated as shown below.
Q: calcualate the pH of a 0.15 M solution of pyruvic acid ka of pyruvic acid is 4.1x10^-3
A: Given: Molarity or concentration of pyruvic acid = 0.15M Ka of pyruvic acid = 4.1 × 10-3
Q: What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid…
A: Given that , Initial concentration of valeric acid = 0.32 M Dissociation constant , Ka = 1.44×10-5…
Q: The acid constants of the polyprotic acid НЗASO4 are К_a1 %3D 5х10 ^-3, К_а2 - 8х10^-8, К_а3 %3D…
A:
Q: Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8 x 10-5.
A: Interpretation: The pH of a 0.800 M NaCH3CO2 solution is to be determined.
Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.468 M methylamine (a weak base…
A: Ch3NH2 is weak base so will not break into ions completely upto 95% in the water. so we have to use…
Q: A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 7.2 x 10-4 M. What…
A: Assuming the weak acid is HA Hence the ionization reaction is HA (aq) + H2O (l) ----> H3O+ (aq)…
Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?
A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…
Q: The weak base colloquially known as Tris, and more precisely as tris(hydroxymethyl)-am inomethane,…
A: Buffer solution is the solution which resist to change the pH on the small addition of acid and base…
Q: CH;NH, is a weak base (Kp = 5.0 × 104), so the salt CH,NH,NO, acts as a weak acid. What is the pH of…
A: The pH of salt of strong acid and weak base can be calculated by using formula
Q: The pOH of an aqueous solution of 0.313 M acetylsalicylic acid (aspirin), HC9H704-
A:
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: Calculate the pH of a 0.100 M NaCH 3CO 2 solution. Ka for acetic acid, CH 3CO 2H, is 1.8 × 103.
A:
Q: When 0.040 mol of propionic acid, C2H5CO2H, is dissolved in 700 mL of water, the equilibrium…
A: Molarity is solution expressed as the number of moles of solute per litre of solution. Equilibrium…
Q: a) A 0.10 Maqueous solution of propanoic acid, CH3CH2COOH, has a pH of 2.93. What is the value of…
A: Hi since you have posted multiple questions, we will answer the very first question. Kindly repost…
Q: The ionization constant (Kb) of aniline (C6HSNH2) is 2.35 x 10-5, If 7.285 grams of aniline is…
A:
Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25oC is 4.48. What is the value of…
A: The concentration of HBrO solution = 0.55 M. pH of aqueous HBrO solution = 4.48.
Q: The acetate ion is the conjugate base of the weak acid acetic acid. The value of K, for CH3C00", is…
A: Here Kb is given for acetate ion so reaction start with acetate ion
Q: The value of Ka for acetic acid , CH3COOH , is 1.80×105. Write the equation for the reaction that…
A: The acids which having the lower pH then the acids will be strong whereas having higher pH value…
Q: What is the pH of a 1.00 x 10^-9 molar solution of KCl?
A: KCl is a salt of strong acid (HCl) and strong base (KOH).
Q: A 0.437 M solution of a weak base has a pH of 11.94. What is the base hydrolysis constant, Kp, for…
A:
Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…
A:
Q: at 25 degrees celcous, the Ka of HCO2H is 1.77 x 10^-4. What is the Delta G naught in kj/mol for…
A: Given : Ka of HCO2H = 1.77 X 10-4 And temperature = 25 oC
Q: The hydroxide ion concentration of an aqueous solution of 0.429 N acetylsalicylic acid (aspirin),…
A:
Q: Calculate the concentrations of all species in a 0.300 M NaCH, COO (sodium acetate) solution. The…
A:
Q: The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous…
A: Given: The ionization constant of the lactic acid = 1.36×10-4 Mass of lactic acid= 20.0g Volume of…
The hydronium ion concentration of an aqueous solution of 0.441 M acetylsalicylic acid (aspirin), HC9H7O4, (Ka = 3.00×10-4) is
[H3O+] =
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
- Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
- The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explain8. (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)Calculate the pH and the pOH of these solutions: (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH = pOH =
- (a) Calculate the percent ionization of a 0.20 M solution of monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10^-4. (b) The pH of gastric acid 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 0.20 M. Calculate the percent ionization of the acid under these conditions.A student is provided with a 0.1 M stock solution of NaOH. Student was then asked to mix 50.0 mL of this stock solution of NaOH with 450.0 mL of water to prepare a dilute solution of NaOH. (A) Calculate the molarity of the diluted solution. (B). Calculate the hydronium ion concentration, [H3O+] in the final diluted solution. (8 points) (C ) Calculate the pH of the diluted NaOH solution. (D) Is the final diluted solution acidic, basic or neutral?The pH of an acetic acid (Ka = 1.75 x 10−5) solution is 3.14. What is the concentration of acetic acid in molarity?
- What is the hydronium-ion concentration of a 1.76 x 104 M solution of p-bromobenzoic acid, BrCgH4 COOH, for which Ka = 1.00 x 10-42 [H3O+]=| |мThe pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) isDetermine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.