Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3 with deonised water.

Q: what volume of sodium sulfate 0.1 M and how many grams of sodium hydrogen sulfate (NaHSO4 . H2O)…

A: : Let V liter be the volume of the sodium sulfate solution that is needed. Let m be the mass of…

Q: How the aqueous chemistry of amphoteric hydroxides involves precipitation, complex-ion formation,…

A: The aqueous solution is the one in which the solvent is water. Different chemical reactions can be…

Q: 1. Consider a solution of NaHA for which F = 0.050 mol L¹, K₁1 = 4.70 x 10³ and K₁2 = 1.80 x 10-10,…

A:

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: A solution is prepared at 25 °C that is initially 0.35 M in propanoic acid (HC,H,CO,), a weak acid…

A: Given: Concentration of propanoic acid = [HA] = 0.35 M Concentration of potassium propanoate = [A-]…

Q: The Ka of propionic acid (HPro) is 1.3 x 105. Which of the following statements is true about…

A:

Q: Determine the pH level of a solution that has 0.05385 M of Pyridine, given that the Kb of pyridine…

A: Given, Concentration of the Pyridine solution (C) = 0.05385 M  Kb for pyridine = 1.620 x 10-6 Note:…

Q: What is the pH of a 1.75 M solution of KX (Kb of X is 1.22 x 10°) (Please show the final result with…

A: Answer:  9.66 Weak base can't dissociate completely, it's  pOH = 1/2 (PKb - logC)

Q: Calculate the acid dissociation constant Ka of a 0.2 M solution of weak acid that is 0.1% ionized is

A: Given, A solution of weak acid that is 0.1% ionized.

Q: TRIS (also known during medical use as THAM) is an organic compound used extensively in biochemistry…

A: "pH" tends to exhibit the actual potential of H+ ions in specified solution. The solution exhibiting…

Q: Calculate the fraction of the weak base in each of its forms at pH 9.62.

A:

Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: whats the kb if the pH of a 1.2 M aq soln of base A at 298 K is 12.32?

A:

Q: The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 :will be respectively…

A: Kh=kWkC pH + pOH = 14  From Ostwald's dilution law ,  pOH=-logkbxc Where c is the concentration of…

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8,…

A: The question is based on the concept of chemical equilibrium. We have to calculate pH of the given…

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 of a solution prepared by mixir (Ka-6.46 x 105) with 5.00 mL of 0.200 M NaO…

A:

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: In theory the pH of distilled water will be 7 or slightly less…why?

A: pH is a measure of the amount of H+ ions in a solution. pH = - log [H+]

Q: Give the pH  of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10

A: Given data :  1.Concentration of C6H5O- = C = 0.005M  2. Ka = 1.0 × 10-10

Q: Given that the acid dissociation constant for benzoic acid (HOBz) is Ka= 6.5 x 10^−5. Calculate the…

A: Recall the dissociation of benzoic acid      HOBzaq+H2Ol→OBz-aq+H3O+aq  Acid dissociation…

Q: Calculate the pH of a solution of 0.1421 M KCH2ClCO2 if Ka = 1.400e-3 for CH2ClCO2H?

A:

Q: Calculate the pH of a 0.75 mol L─3 solution of ethanoic acid at 298 K. Given Ka = 1.7 × 10─5

A: Welcome to bartleby ! We have to calculate pH .

Q: Galaulate the PH and the Pott FOR 9.6M solution OF MH₂ инз K. FOR NH3=1.97105

A: Here we are required to find the pOH and pH of 0.6M of ammonia solution

Q: A decrease of PH by 3 implies

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: Calculate the pH of 0.564 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10-5)

A:

Q: B) For the following sets of compounds, place the compounds in order of increasing acidity, and…

A: The acidity for a given compound depends upon the number of -I group attached to the system. More…

Q: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 × 10¯°. Calculate the pH of a…

A:

Q: What is the percent ionization of nitrous acid in a solution that is 0.230 M in nitrous acid (HNO2)…

A: The percent ionization of nitrous acid in a solution is to be calculated

Q: The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is

A:

Q: What is the ionization constant at 25 °C for the weak acid (CH3)2NH2+,the conjugate acid of the weak…

A: Formula for relationship between ka and kb is  ka*kb= 10-14 Ka= 10-14/kb Ka= 10-14/5.9x10-4 Ka=…

Q: Determine the base ionization constant (in x 10-5) of a 0.0925 g sample of a weak base (molar mass =…

A: Given :- Mass of weak base = 0.0925 g Molar mass of weak base = 17.03 g/mol Volume of water = 100 mL…

Q: 10.06 cm3 of the stock 0.100 mol dm-3 solution of NaOH was required to fully neutralise 49.5 mg of a…

A: Volume of NaOH = 10.06 cm3  Molarity of NaOH = 0.100 mol dm-3  Mass of diprotic acid (H2A) = 49.5 mg…

Q: CH3NH2 is a weak base (Kb = 5.0 x 10-4 ) and so the salt CH3NH3NO3 acts as a weak acid. What is the…

A:

Q: Calculate the pH and the concentrations of all the species present in 0.010 M of Carbonic acid…

A:

Q: What is the pH of a 1.63 M solution of XOH, a weak monobasic compound (Kb = 1.7 x 10^-9)?

A: Given data in above Concentration of XOH = 1.63 M  Kb = 1.7 ×10-9

Q: Calculate pH and pOH of the: 0.5M aniline (C6H5NH2) solution (Kb= 3.8 x 10-10)

A: Given,  [C6H5NH2] = 0.5 M  Base dissociation constant of C6H5NH2 = 3.8 x 10-10 pH and pOH = ?  Base…

Q: The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20…

A: #(a): H2SO4 is a diprotic acid. The dissociation equations are: H2SO4(aq) ----> HSO4-(aq) +…

Q: The acid dissociation constant for acetic acid (HC2H3O2, commonly abbreviated HAc) is 1.8 x 10-5.…

A: Given, Acid dissociation constant, Ka = 1.8*10-5. Molarity of acetic acid solution = 0.10M. The…

Q: At a temperature of 298K the value of Ka for ethanoic acid is 1.70 * 10Smoldm3. c. Calculate the pH…

A: The given data contains, Ka of ethanoic acid =1.70×10-5moldm-3Concentration of ethanoic acid =0.350…

Q: Determine the pH of a 0.530 M solution of carbonic acid that has an acid dissociation constant of…

A:

Q: What is the pH of a 0.420 M solution of C5H,NHB (Kb of C5H,N is 1.7 × 10-9)?

A: Given:: [C5H5NHBr]=0.420 M =concentration of salt=c Kb of C5H5N = 1.7×10-9 pH=?

Q: The pH and Kh of O.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 will be respectively equal…

A: Value of pH is used to measure extent of acidity or basicity of a solution. At room temperature,…

Q: Calculate the isoionic pH of 6.022 x 1021 molecules of thereonine in 500 mL of solution. (For…

A:

Q: Calculate the pH of an aqueous solution of 1.00 M iodic acid at 298K.

A: The equation for the dissociation of Iodic acid is,

Q: The base protonation constant K, of allantoin (C,H,N,0,NH,) is 9.12× 10¯°. 9. 4 Calculate the pH of…

A: Given information: Concentration = 1.3 M

Q: Calculate the pH of a 0.05 mol dm3 CH;COOH solution: the dissociation constant Ka for CH;COOH is…

A: An acid which will not dissociate completely to furnish hydrogen ion is called weak acid

Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 × 10". Calculate the pH of a…

A:

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.