A 0.25-mol sample of a weak acid with an unknown pKa   is combined with 10.0 mL of 3.00 M KOH and the resulting solution is diluted to 1.500 L. The measured pH of the solution is 3.85. What is the pKa  of the weak acid?

Q: 0.400 M

A: A) mmoles of Acid = 60.0mL • 0.355molL-1 = 21.3mmol  B) mmles of Base = 75.0mL • 0.400molL-1 =…

Q: A 50.0 mL sample of 0.100 M NH, is titrated with 0.100 M HBr. What is the most likely pH of the…

A: Answer :- 2.041  pH = 2.041…

Q: In a titration experiment of a 25.00 ml of 0.100 M CH3CO2H with 0.100M NaOH, 12.50 mL of NaOH were…

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Q: calculate the pH of a solution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 0.10 L…

A: The pH can be calculated as,

Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in…

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Q: The pKa of hypochlorous acid is 7.530. A 52.0 mL solution of 0.114 M sodium hypochlorite (NaOCl) is…

A:

Q: You have a 0.500 L buffer solution composed of 0.47  M formic acid (HCOOH, Ka = 1.77 x 10¯4) and…

A: The acid ionization constant for acid is 1.77×10 -4.

Q: 10mL of a 0.28 M solution of acetic acid, Ka = 1.8 x 10-5,  is added to a 20mL of 0.18 M solution of…

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Q: 4. Calculate the mass of sodium acetate that must be added to 1.50 L of a 0.456 M acetic acid (Ka =…

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Q: 130 mL of 0.7 M solution NaHCO3 is titrated by 0.5 M HCIO3 (Kp = 2.4 x 108). (i) What is the pH…

A:

Q: Calculate the pH values and draw the titration curve for the titration of 500 mL of 0.010 M acetic…

A: The above titration is of a weak acid and strong base.  Number of moles of CH3COOH initially =…

Q: Consider the titration of a 40.0 mL of 0.189 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH.…

A: Given:   The volume of HA is 40.0 mL. The concentration of HA is 0.189 M. The value of Ka is…

Q: Calculate the mass of Cd (OH)2 that will dissolve in a buffer made by combining 200.0 mL of 5.0 M…

A:

Q: 5. If the pH of the saturated solution Mg (OH)2 is equal to 10.5, calculate the Ksp of this salt.

A:

Q: Consider the titration of a 50.0-mL sample of 0.0500 M HCI with a 0.0250 M NaOH solution. What is…

A:

Q: What is the pH of a buffer made from 0.350 mol of HBRO (Ка 3 (Ka = 2.5 x 10°) and 0.080 mol of KBRO…

A: Given : Moles of HBrO = 0.350 mol. Moles of KBrO = 0.080 mol. Ka of HBrO = 2.5 X 10-9  And volume of…

Q: A buffer solution that is 0.458 M in HCN and 0.458 M in KCN has a pH of 9.40. The addition of 0.01…

A: The buffer solution consists of a weak acid (HCN) and the salt of weak acid and strong base (KCN).…

Q: A 96.0 mL volume of 0.25 M  HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 48.0…

A: Given: Concentration of HBr = 0.25 M Concentration of KOH = 0.50 M Volume of HBr solution = 96.0 mL…

Q: A buffer is prepared by mixing 35.2 mL of 0.183  M NaOH with 141.2  mL of 0.231 M acetic acid. What…

A: Given: Concentration of acetic acid = 0.231 M Volume of acetic acid solution = 141.2 mL = 0.1412 L…

Q: Question attached

A: Given,  [C5H5N] = 0.170 M  Volume = 25.0 mL = 0.025 L  [HBr] = 0.170 M  pH = ?

Q: Calculate the molar solubility of Ca(OH) in a solution buffered at pH = 10, if the %3D solubility…

A:

Q: A 27.0-mL solution of 0.120 M CH3COOH is titrated with a 0.230 M KOH solution. Calculate the pH…

A:

Q: Consider the titration of a 60.0 mL of 0.317 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH.…

A: Chemical equation: HA (aq)  +    KOH (aq)  ------->   KA (aq)   +   H2O Number of mmols of KA…

Q: A 50.0 ml sample of 0.200 M HNO2 (weak acid) is titrated with 0.400 M KOH. Calculate the pH after…

A: Neutralization reaction is a type of chemical reaction that occurs between acid and base resulting…

Q: -1 A 75.0-mL volume of 0.200 mol L NH3 (Kp = 1.8 × 10-3) is titrated with 0.500 mol L HNO3.…

A:

Q: Consider the titration of a 40.0 mL of 0.153 M weak acid HA (Ka = 2.7 x 10-8) with 0.100 M LİOH.…

A:

Q: 0.0 mL sample of 0.100 M ammonium chloride (NH₂, K, 5.70 x 10 10) is titrated with 0.100 M NaOH.…

A:

Q: Calculate the pH at the equivalence point for the titration of 0.100 M methylamine (CH, NH,) with…

A: Consider the reaction of titration of methylamine with HCl is as follows: CH3NH2 + HCl ⇌ CH3NH3+ +…

Q: A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCI and 2 drops of…

A:

Q: - If a 1.0 M solution of NaOH is slowly titrated (dripped) into a 0.050 M solution of Mn2 (aq), what…

A: Given : Concentration of Mn2+ = 0.050 M  And pH of solution becomes 8.00  Since pH = 14 + log[OH- ]…

Q: A 28.0-mL solution of 0.120 M CH3COOH is titrated with a 0.220 M KOH solution. Calculate the pH…

A:

Q: Calculate the pH of the solution that results from the addition of 0.040 moles of HNO3 to a buffer…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: A 26.9 mL sample of 0.375 M diethylamine, (C2H5)2NH, is titrated with 0.258 M nitric acid.The pH…

A:

Q: 8. State True or False. In the titration of a weak acid with a strong base, pKa of the weak acid…

A: The equivalence point is the point where the number of moles of acid and base is approximately…

Q: Calculate the mass of Cd(OH)2 that will dissolve in a buffer made by combining 400.0 mL of 8.0 M NH3…

A: Henderson hasselbalch equation: pOH=pKb+log[conjugate acid][weak base]

Q: In the titration of 50.0 ml of 0.1 M formic acid (ka- 1.8x 10) with 0.1M NAOH, what will be the pH…

A:

Q: Consider the titration of 50.0 mL of 0.134 M HNO3 with 0.0500 M KOH. What is the initial pH of HNO3…

A: pH = -log [H3O+]

Q: Hi, I need help

A: The reaction taking place is,

Q: You have 500mL of a solution containing 0.20M acetic acid (CH;COOH) and 0.30M sodium acetate…

A: Prior to the addition of NaOH, [CH3COOH] = 0.20 M [CH​​​​​​​3​​​​​​​COO​​​​​​​-] = 0.30 M On…

Q: A buffer solution that is 0.470 M in HClO and 0.470 M in KCIO has a pH of 7.46. The addition of 0.01…

A:

Q: A 5.55-g sample of a weak acid with Ka = 1.3 × 10-4 is combined with 5.00 mL of 6.00 M NaOH and the…

A: The general reaction between NaOH and diprotic acid is as follows,

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has: Concentration of NH4Cl/NH4+ = 0.182 M Concentration of NH3…

Q: Calcium hydroxide (Ca(OH)a) is a strong base. Its solubility is about 0.74 g/L at 25°C. 1. For a…

A:

Q: A buffer solution that is 0.320 M in HC1O and 0.320 M in KC1O has a pH of 7.46. The addition of 0.01…

A: Effect of added base or acid in a buffer solution is calculated from Henderson-Hasselbalch equation:…

Q: A titration is performed in which 0.10 M LIOH is added to a 200.0 mL sample of 0.40 M HF. What is…

A: HF is a weak acid it reacts with LiOH which is a strong  base and gives fluoride ion. Now this…

Q: A titration process is done by using 0.2M of 20 ml of third analytical group main reagent solution…

A: Let V  volume is used when nitric acid is used . Nitric acid donate only one H+ ion and H2SO4 donate…

Q: A titration is performed in which 0.14 M KOH is added to a 150.0 mL sample of 0.39 M HI. What is the…

A: PH of KOH can be calculated as follows

Q: Consider the titration of a 40.0 mL of 0.189 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH.…

A: Number of moles of weak acid = 0.04 L × 0.189 M = 0.00756 mol. Number of moles of LiOH = 0.1 M × 0.1…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for