chemist named Ciara titrates X mL of a 0.7633 M hypochlorous acid (HA) solution with 0.3245 M solution of LiOH at 25 degrees Celsius. Calculate the pH at equivalence. The Ka of hypochlorous acid is 3.16 x 10-8.

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 525-mL buffer solution is 0.367 M in acetic acid (CH3COOH) and 0.367 M in sodium acetate…

A: We have to calculate the initial pH and pH after adding given amount of acids and bases.

Q: A sample of nitric acid, HNO3 is titrated with NaOH. Which of the following would be the best…

A: This is a type strong acid vs strong base titration

Q: Consider the titration of a 60.0 mL of 0.295 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH.…

A:

Q: Two acids are mixed in solution: 0.20 M of HBr and 1.50 M of HBRO (Ka = 2.3 x 10-9). What is the…

A: HBr is a strong acid while HBrO is weak acid and therefore, the resulting pH will be due to HBr,…

Q: buffer solution is made that is 0.319 M in HCN and 0.319 M in NaCN. (1) If Ka for HCN is 4.00×10-10…

A: Here the Ph will be equal to Pka.

Q: i. First, identify the acid. It's either H2PO41 or HPO42. The acid is because it has the most acidic…

A: Answer-1 H2PO4- H2PO4- because it has more number of acidic hydrogens, that's why it will lose it…

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10¬4,…

A:

Q: A buffer solution was made by mixing equal volumes of 0.20 mol/L solutions of acetic acid and sodium…

A:

Q: 55.00 mL of a solution of 0.1325 M maleic acid is titrated with 0.1000 M NaOH. What Is the pH when…

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 LiOH.…

A:

Q: A 105.2 mL sample of 0.100 M methylamine ( CH3NH2; Kb = 3.7 x 10-4) is titrated with 0.270 M HNO3.…

A: Answer:- This question is answered by using the the simple concept of calculation of PH during the…

Q: Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONa.

A: Ka for acid = 1.8 x 10-5  [CH3COOH] = 1.0 M [CH3COONa] = 1.2 M  PH = ?

Q: CH3 O H3C-CC-OH H H3CH_2_2 CH3 C-OH H+ Heat

A:

Q: The graph here shows the pH curve for the titration of 25.00 mL of a 0.100-M monoprotic acid…

A: Acid base titration is indicator based titration. It gives different colour at different pH value.…

Q: Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that is 0.28…

A: The objective of the question is to calculate the pH of two different solutions using the…

Q: A buffer solution is made that is 0.319 M in HCN and 0.319 M in NaCN. (1) If Ka for HCN is…

A:

Q: What is the pH of a buffer solution that is 0.159 M in hypochlorous acid (HCIO) and 0.121 M in…

A: Given: Concentration of hypochlorous acid (HCIO)=0.159 M Concentration of  sodium hypochlorite…

Q: What is the pH of a weak base-strong acid titration when 20.0 mL of 0.56 M of NaOCl (Ka = 3.0*10-8)…

A:

Q: A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of…

A: The objective of this question is to calculate the pH of a buffer solution after adding a certain…

Q: A 0.15 M solution of HIO2 is being titrated with a 0.15 M solution of NaOH. 20.0 mL of the HIO2 is…

A:

Q: Calculate the pH of a buffer solution that is 0.41 M in HOCl and 0.50 M in NaOCl. [Ka(HOCl) = 3.24 x…

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: At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The…

A: The pH of the resulting solution of metal hydroxide M(OH)2 when mixed with pure water = 10.20pH +…

Q: potassium hydroxide. (Ka (HBrO) = 2.0 x 10-9) a. What is the initial pH of the solution? HBrO + H₂O…

A: a)when 0.0 mL of KOH is addedHBrO dissociates as:HBrO          ----->     H+   +  BrO-0.8…

Q: Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25°C. K for HCN 6.2×10-10, Part…

A: The objective of this question is to calculate the pH at different stages of a titration process.…

Q: 20.0 mL of 0.075 M aqueous solution of lactic acid CH3CH(OH)COOH, a monoprotic acid, is titrated…

A: volume of NaOH at equivalence point  pH at equivalence point  pH after adding 5.0 mL of NaOH

Q: The pH at the equivalence point in the titration of 0.10 M HF (k_{a} = 6.3 * 10 ^ - 4) with 0.10 M…

A:

Q: A buffer solution is made that is 0.418 M in HCN and 0.418 M in NaCN. K₂ for HCN is 4.00 x 10-¹0,…

A: Given,Molarity of HCN = 0.418 MMolarity of NaCN = 0.418 MKa of HCN = 4.00 x 10-10 moles of KOH =…

Q: Consider the titration of 25.00 mL of 0.100 M hydrofluoric acid, HF, with 0.100 M NaOH. What is the…

A:

Q: You are to prepare exactly 100 mL of 0.200 M acetate buffer, pH 5.00, starting with pure liquid…

A: Formula used  Handerson- Hasselbalch equation  pH = pKa + log[CH3COONa/CH3COOH]  pH= 5.00 , pKa =…

Q: Calculate the pH of a buffer solution that contains 300 mL of 0.60 M CH3COOH and 200 mL of 0.60 M…

A: We have to calculate the pH of solution.

Q: Strong base is dissolved in 665 mL of 0.200 M weak acid (K₁₂ = 4.73 × 10¯5) to make a buffer with a…

A: In the given question strong base was dissolved in weak acid to make a buffer but initially only…

Q: A solution made by mixing 105.00 mL of 1.050 M CH3COOH with 35.00 mL of 0.750 M NaOH. For…

A: A buffer resists a considerable change in pH when a small amount of acid or base is added to it. The…

Q: A 80.00 mL solution initially contains 0.300 M HCN and 0.200 M KCN. What is the new pH after 1.0 mL…

A: To find the new pH after adding 1.0 mL of 2.5 M HCl to the solution, we need to consider the effect…

Q: Consider the titration of 50.0 mL of 0.20 M NH3 (Kµ = 1.8 × 10−5) with 0.20 M HNO3. Calculate the pH…

A: we  have:  molarity of HNO3 = 0.2 M  Volume of HNO3 = 50 mL  Molarity of NH3 = 0.2 M  Volume of NH3…

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.