15) How many milliliters of 0,225M HaPO, WOuld be needed to react exactly with 20.0mL of 0.135M NaOH? H3PO4(aq) +3NAOH(aq) →Na3PO4(aq) + 3H20(1)
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- According to the following reaction how many ML of 1.245 M LiOH is needed to neutralize 32.02 ML of 1.065 M H3PO4? reaction: H3PO4(aq)+3LiOH(aq)--->3H2O(l)+Li3PO4(aq)A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).14) How many milliliters of 0.225M HCl would be needed to react exactly with 20.0mL of 0.135M NAOH? HCl(aq) + NaOH(aq) →NACI(aq) + H2O(1)
- Use the equation below to calculate the following: 2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) (a) the grams of Na2SO4 that can be obtained from 25 mL of 0.050 M NaOH (b) the volume of 0.250 M H2SO4 needed to react with 25.5 mL of 0.750 M NaOH (c) the molarity (M) of the NaOH solution when 48.20 mL react with 35.72 mL of 0.125 M H2SO41. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid, H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is the concentration of the phosphoric acid solution using the results that were obtained? K Given: H₂PO4(aq) + 3NaOH(aq) - Na3PO4(aq) + 3H₂O(1) Initial Buret Reading (mL) Final Buret Reading (mL) Volume Base Added (mL) 2 => Na Mg Rb Sr 2.92 M Cs Ba 0.55 M 1.21 M Be 0.97 M 1.76 M Ca Sc 3.11 M Ra La 91 AM Hf Ac Trial 1 0.3 14.2 TI Zr Nb Mo Tc [81 $4 Cr Mn Fe Re Os Rf Db Sg Bh Hs Periodic Table of the Elements T Trial 2 14.2 A Basic D 30.0 Symbol 10 77 78 224, Co Ni Cu Zn Ga B 14 Neble Gas Trial 3 30.0 43.9 Ru Rh Pd Ag Cd In Sn Sb Te M с N Expe 201 VIA Sm Nd Pm Eu Gd Dy Ho "Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 15 VIA M He Ge As Se Br Kr Xe Pt Au Hg Ds Rg Cn Uut FI Uup Lv Uus Uuo Ne "Er Tm YbA chemist titrates a 25.0 mL sample of 0.239 M benzoic acid (C6H5COOH) against a 0.100 M solution of NaOH.The overall reaction is shown by the equation below: C6H5COOH(aq)+NaOH(aq)C6H5COONa(aq)+H2O(l) The Ka value for benzoic acid is 6.28 × 10–5. Calculate the pH at the start of the titration, before any NaOH has been added. Give your answer correctly to two places after the decimal.
- Fill in only the appropriate boxes in the ICE table below as you would to answer the following question: What is the concentration of H30* in a 0.2 M solution of HCIO3 in water? (Only fill in the ICE table; actual calculation of [H3O+] is not required). H20(1) HCIO,(aq) I | C CIO;"(aq) E HCIO,H*(aq) H;O*(aq) || OH"(aq) 0.2 0.2-x | 0.2+x -X +X X | Please put an answer in each box. 11Complete the changes in concentrations for each of the following reactions:(a) BaSO4(s) ⟶ Ba2+(aq) + SO4 2−(aq) x _____(b) Ag2 SO4(s) ⟶ 2Ag+(aq) + SO4 2−(aq) _____ x(c) Al(OH)3(s) ⟶ Al3+(aq) + 3OH−(aq) x _____(d) Pb(OH)Cl(s) ⟶ Pb2+(aq) + OH−(aq) + Cl−(aq) _____ x _____(e) Ca3(AsO4 )2(s) ⟶ 3Ca2+(aq) + 2AsO4 3−(aq) 3x _____A 56.01 mL sample of HCN was neutralized by exactly 35.04 mL of 0.1233M LiOH. What was the molarity of HCN?HCN(aq) + LiOH(aq) ↔ LiCN(aq) + H2O(l)
- A 0.7500 g sample of a phosphoric acid (H3PO4) solution with unknown concentration requires 30.00 mL of 0.3375 M NaOH to reach the end point. Calculate the %(m/m) concentration of the phosphoric acid in the unknown solution. H3PO4(aq) + 3NaOH(aq)---> K3PO4(aq) + 3H2O(l)A railroad tank car derails and spills 26 tons of concentrated sulfuric acid (1 ton = 907.185 kg). The acid is 98.0% H2SO4 with a density of 1.836 g/mL.(a) What is the molarity of the acid? (b) Sodium carbonate, Na2CO3, is used to neutralize the acid spill. Determine the kilograms of sodium carbonate required to completely neutralize the acid. (c) How many liters of carbon dioxide at 18°C and 745 mm Hg are produced by this reaction?What is [H3O+ ] (in M) in a solution of 0.072 M HBrO2 and 0.035 M NaBrO2? (Assume Kw = 1.01 ✕ 10−14.) HBrO2(aq) + H2O(l) H3O+(aq) + BrO2−(aq) Ka = 3.7 ✕ 10−4
