When doing titration to an acid with NaOH, instead of using HCl, you used H2SO4 instead. Would you use the same amount of H2SO4?   Yes. The reaction is the same since both are strong acid. No. The reaction depends on the concentration. Yes. The reaction does not matter with the type of an acid. No. The reaction does not follow the same ratio.

1. Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc).  Ka for HAc is 1.8x10 -5.  What is the initial pH of the solution (before the titrant is added)?

What is the concentration of manganese ions in a saturated solution of manganese sulfide? 4.0✔ M Calculate the pH of a saturated solution of lead hydroxide. See the Solubility Product Constant Table. 4.0✔ Substance Ksp at 25 °C Aluminum Al(OH)3 1.9 x 10-33 Barium Ba(OH)2 BaCO3 BaSO4 1.1 x 10-10 Ba3(PO4)2 3.4 x 10-23 Cadmium Cd(OH)2 CdCO3 CdS Calcium Ca(OH)2 CaCO3 5.0 x 10-3 8.1 x 10-⁹ 5.5 x 10-6 4.8 x 10-9 Ca3(PO4)2 1.0 x 10-26 CaF2 3.9 x 10-11 2.5 x 10-14 5.2 x 10-12 8.0 x 10-27 Chromium Co(OH)2 Cr(OH)3 6.3 x 10-31 Cobalt COS 1.6 x 10-15 4.0 x 10-21 Copper Cu(OH)2 Cu₂S CUCO3 CuS Iron Fe(OH)2 FeS Fe(OH)3 FePO4 Lead Pb(OH)2 PbF2 PbCl₂ PbBr₂ Pbl2 PbCrO4 PbSO4 PbS 2.2 x 10-20 1.6 x 10-48 1.4 x 10-10 6.3 x 10-36 Mg(OH)2 8.0 × 10-16 6.3 x 10-18 2.5 x 10-39 9.9 x 10-29 2.8 x 10-16 3.7 x 10-8 1.7 x 10-5 6.3 x 10-6 6.5 x 10-⁹ 1.8 x 10-14 1.7 x 10-8 8.4 x 10-28 Magnesium 1.8 × 10-11 Manganese Mn(OH)2 MnCO3 MnS Nickel NI(OH)2 Silver AgCl AgBr Agl AgCN Ag₂S Ag₂ CrO4 Ag3PO4 Tin Sn(OH)2 SnS Zinc…

1.00 x 10-² A student was titrating a solution of HC4H7O₂ with a Sr(OH)2 solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. Before (mol) Change (mol) After (mol) NEXT > 40.0 mL of a 0.200 M HC4H7O2 solution was titrated with 100 mL of 0.100 M Sr(OH)2 (a strong base). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. 0 -1.00 x 10-² 1 HC4H-O₂(aq) + 0.100 1.20 x 10-² 0.200 OH-(aq) -1.20 x 10-² 2.00 x 10-³ 2 2.00 x 10-² H₂O(l) + -2.00 × 10-³ -2.00 x 10-² C4H7O₂ (aq) 8.00 x 10-³ RESET -8.00 x 10-³

Consider the titration of a 60.0 mL of 0.321 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH. 1. What is the pH before any base has been added? 2. After 30.0 mL of KOH have been added, identify the primary species left in the solution. 3. After 30.0 mL of KOH have been added, what would the pH of the solution be? 4. After 75.0 mL of KOH have been added, identify the primary species left in the solution. 5. After 75.0 mL of KOH have been added, what would the pH of the solution be?

For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4-  + H2O ⇌  HPO42-  + H+  pKa= 7.21  (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)

Titrating ascorbic acid with iodine is what type of titration? HO. HO. + 2 HI HO 3x-3x= h + HO HO OH Iodine Ascorbic Acid Dehydro-Ascorbic Acid O An acid-base neutralization titration, because iodine is a strong acid OA redox titration, because iodine acts as an oxidizing agent OA redox titration, because iodine acts as a reducing agent An acid-base neutralization titration, because ascorbic acid is a weak base

7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?

2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH COOH with 9.00 mL of 0.080 M NaOH. a. Calculate the moles of CH COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH₂COOH and CH COO present in the buffer solution. c. Calculate the concentration of CH COOH and CH COO in the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH COOH K₂ = 1.8 x 10.

A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka’s for KHP are 1.12 x 10-3 and 3.90 x 10-6   Calculate the pH of this solution before adding any NaOH. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? Calculate the pH of the solution after 100. ml of NaOH have been added.