Q: HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a…
A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.054M in…
Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…
A: We will calculate the number of moles of each reactant and then draw ICE table to calculate pH of…
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: 1) Calculate the pH (aq., 25 °C) of a 0.073 M Novocaine (C13H21O2N2CI) solution, which is the salt…
A: Solving only first question in accordance with guidelines. We will first draw ICE table and then…
Q: Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4…
A: Given- Concentration of CH3NH2 = 0.35 M Kb = 4.4 × 10-4 To find - pH of solution Formula- pH = - log…
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 0.350 M triethylamine, (C2H5)3N, solution? Kb for triethylamine is…
A: Given, 0.350 M triethylamine Kb for triethylamine is 5.3 *10-4
Q: What is the pH of a 0.232 M solution of ammonia, a weak base with a K of 1.7 x 10-5?
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and…
A: We will calculate pH
Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?
A:
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: What is the pH of an aqueous solution of 0.159 M sodium cyanide (NaCN)? (Kb of CN- = 2.5 x 10-5)
A: Given, The concentration of sodium cyanide (NaCN) = 0.159 M Kb for CN- = 2.5 x 10-5. pH is the…
Q: What is the pH of a 0.0490 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?
A:
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: what is the ph of a 0.85 M solution of pyridine (C5H5N, Kb = 1.70 x 10 ^-9)
A: Pyridine is a weak base. pOH of a weak base. pOH = -log [OH-] pH = 14 - pOH For a weak base like…
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 0.150 M solution of acetic acid (pKa=4.75) at 25 degree celsius?
A: Given, the concentration of acetic acid =0.150 Mand pKa of acetic acid =4.75 at 25 °Cwe are asked to…
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 the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 10*)?
A: A numerical problem based on pH of the weak base, which is to be accomplished.
Q: Calculate the pH of 0.564 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10-5)
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: 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: Calculate the pH of a 0.100 M CH 3NH 3CI solution. Kb for methylamine, CH 3NH 2, is 3.7 × 10 4.…
A:
Q: Calculate the pH of a 0.021 M NaCN solution at 25 degrees Celsius. Ka (HCN) = 4.9 x 10^(-10). You…
A: Given, Concentration of NaCN solution = 0.021M. Ka(HCN) = 4.9*10-10. The hydrolysis reaction of NaCN…
Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?
A:
Q: What is the pH of a 0.0580 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1º)?
A:
Q: What is the pH of a 0.0100 M solution of analine (C6H5NH2) , a weak base. Kb= 4.0 x10-10
A: The chemical equation for aniline can be written as: This equation shows that aniline is a base,…
Q: 5c. What is the pH of a solution which is 0.0400 M in potassium isocyanate (K* CNO") and 0.0300 M in…
A: Given, [K+CNO-] = 0.0400 M [HOCN] = 0.0300 M As , K+CNO- is a salt it remains as…
Q: What is the pH of a 0.0310 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 10-10)?
A: Answer:- This question is answered by using the simple concept of calculation of pH of weak acid…
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: What is the pH of a 0.75 M solution of sodium cyanide, NaCN? (Kb for CN- = 2.5 x 10^-5)
A: NaCN is a salt of weak acid and a strong base. The pH of a salt of weak acid and strong base can be…
Q: What is the pH of 0.31 M diethylammonium chloride, (C2H5)2NH2Cl. The Kb of diethylamine, (C2H5)2NH,…
A: The pH of the 0.31M diethylammonium chloride is given below
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: What is the pH of a 0.248 M aqueous solution of potasslum acetate, KCH,CO0 at 25 °C? (K, for CH,COOH…
A: 1.) Potassium acetate is a salt of conjugate base of acetic acid. So we would draw ICE table and use…
Q: HClO is a weak acid (Ka=4.0×10−8Ka=4.0×10−8) and so the salt NaClO acts as a weak base. What is the…
A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.029M in…
Q: What is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?
A:
Q: Calculate the pH of a 0.300 M solution of the dibasic compound piperazine, which we will designate…
A: pH is used to determine the concentration of hydronium ion.
Q: 6. What is the pH of a 0.250M solution of methyl amine (CH3NH2, Kb = 4.4 x 104)?
A:
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 0.278 M diethylammonium iodide, (C2H5)2NH2I. The Kb of diethylamine, (C2H5)2NH,…
A:
Q: What is the pH of a 0.0500 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?
A: Given -> Molarity of HCN = 0.0500 M Ka = 4.9 × 10-10
Q: what is the ph of 0.0349 M anilinium hydrochloride (C6H5NH3CI) solution in water, given that K for…
A:
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: Calculate the pH of 0.17 M propanoic acid CH3CH2COOH, found in the sample analysis of sewage water.…
A: We have CH3CH2COOH →CH3CH2COO- + H+ Concentration of propanoic = 0.17 M Ka=1.3 x 10-5
Q: What is the pH of a 0.0680 M solution of hydrocyanic acid, HCN (Ка %3D 4.9 х 10-10)?
A:
Q: ph of 0.10 M NaNO2 (Ka of HNO2 is 4.5 x 10-4 ?
A: Given information: 0.10 M NaNO2 Ka of HNO2 is 4.5 x 10-4
Q: The [H3O+] of Coca-Cola Classic ® is 3.2 x 10-3. What is its pH? Is it acidic or basic?
A: The pH of the given solution can be defined as the measure of its basicity or the acidity. It is…
Q: HClO is a weak acid (?a=4.0×10−8) and so the salt NaClO acts as a weak base. What is the pH of a…
A: An acid is a substance that can furnish the hydrogen ions in the aqueous solution. The weak acid…
What is the pH of 0.836 M anilinium hydrochloride (C6H5NH3CL) solution in water, given that Kb for aniline is 3.83 x 10-4?
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- What is the pH of a 0.120 M solution of aniline (C6H5NH2, Kb = 4.3 x 10 10)?The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.
- Calculate the pH of a 0.591 M aqueous solution of benzoic acid (C6H₂COOH, K₂ = 6.3x10-5). pH =10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, Kb = 4.3x104 that has an initial concentration of 0.20 M? Is it acidic, basic, or neutral solution?If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of hydrazine.
- What is the pH of a 0.1 M solution of methylamine hydrochloride (CH3NH3Cl), if pKb of CH3NH2 = 4?Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³ hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution. Page 4 of 14The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10^–8. (a) The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.
- Calculate the pH of a 0.600 M solution of methylamine CH3NH2. Kb = 4.4 x 10–4Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.644 M solution of N2H4.CH3NH2 is a weak base (Kb = 5.0 x 10-4 ) and so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a 0.0150 M solution of CH3NH3NO3 at 25oC? You must write the reaction of hydrolysis.