you are titrating 50mL of 0.1 M AgNO3 with 0.2750 M NaBr. Calculate pAg at half of the volume necessary to reach the equivalence point, at Ve, and 10mL after Ve. Assume Ksp = 2.15*10^ - 13
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- Consider the titration of 100.0 mL of 0.100 M hydrazine (H2NNH2, K, = 3.0×10-6) by 0.200 M HNO3. Despite the symmetric nature of the hydrazine's molecular structure, it accepts only a single proton from HNO3 in aqueous solution. (Kw = 1.00×10-14) %3D %3D (a) Calculate the pH of the solution after addition of 0.0, 20.0, 25.0, 40.0, 50.0, and 100.0 mL of HNO3 to the solution. (Note: you need to consider the range of applicability of the Henderson- Hasselbalch equation and need to check if water autoionization can be neglected. See Figure 15.18 in the textbook.) (b) Based on your answer to part (a), sketch the titration curve, marking the calculated points and labeling the equivalence and half-equivalence points. (c) Although still weak, ammonia (NH3, Kb = 1.8×10-5) is a stronger base than hydrazine. Sketch the titration curve for 100.0 mL of 0.100 M ammonia by 0.200 M HNO3 on the same axes as your answer to part (b); be sure to label the curve. %3D Note: a qualitative sketch is….. .- V . * CÓ LO x Sona Paychology Research Pa X app.101edu.co Question 9 of 9 Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC4H,O2 is 1.5 x 10-5.. 2 NEXT 1. 3. Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HC4H;O2(aq) + OH (aq) C4H,O2 (aq) (1)O?H Before (mol) Change (mol) After (mol) ORESET 0.200 00L'O c.0L x 00'L- c.0L x 00'7 cOL x 00'7- c-0L x 00'L c.OL x 00'L -7.00 x 103 8.00 x 103 cOL x 00'9 c.0L x 00'9- c.0L x 00'8- MacBook Air esc DD F4 F5 F8 F12 # 2$ 2 delete 6. 7. R P. %31 A K ck S H trol command command optionWhat volume of a 0.0225 solution of potassium permanganate are required to titration 0.461 g sample that is 61.4% sodium oxalate. 2MnO4^- + 5C2O4^-2 + 16H^+ = 2Mn^2+ + 10Co2 + 8H2O
- Consider the titration of 80.0 mL of 0.0200 M NH3 (a weak base; Kb = 1.80e-05) with 0.100 M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH = (b) 4.0 mLpH = (c) 8.0 mLpH = (d) 12.0 mLpH = (e) 16.0 mLpH = (f) 22.4 mLpH =Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 0.10 M H3PO4 with 0.075M NaOH. There will be two of themFor the titration: 30.0mL of 0.150 M NH3 (Kb = 1.8 x 10-5) with 0.250 M HBr Calculate the pH after 20.0mL of HBr are added to the flask.
- 4-Calculate pCl for the titration of 100.0 mL of 0.1000 M Cl¯ with 0.1000 M AGNO3 for the addition of 0.00 and 20.00 mL AGNO3. ptor TOCLR)3(AOYes) SHIFT WODE (SETUP)(1 MtOOMatho) AWA SETUPIOaOaLineo) A SETUPIELinelo) ETUPIOO4CONT) g F9 CLR) O(Setup)O(Yes)help ASAP Compare the two quantities based on the given condition: A solution containing KOH and KHCO3 is titrated with 0.100 M HCl using a one-flask method. I. Volume of titrant from 0.00 mL to the phenolphthalein endpoint II. Volume of titrant from the phenolphthalein end point to the methyl red end point. (a) I < II (b) I = II (c) I > II (d) The two quantities cannot be compared due to insufficient information.1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…
- 3. Calculate the (a) pH (b) pOH (c) percent ionizaton of 0.100 M ammonia. NH3 kb = 1.8x10^-5 4. Give five (5) techniques on how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry. please answer all questions. I don't have questions left so i cannot repost the other questionCalculate pF at the equivalence point of a titration of 20.00 mL of 0.01039 M La (NO3)3 with 0.006338 M NaF.✓ Correct Precipitation will occur when Q2 Kp. You can use this to calculate the concentration of SO needed for precipitation of each compound. CaSO₁: Ag₂SO4 Part B Kap[Ca²+][SO]=2.4 x 10-¹ 2.4 x 105 = (0.20)[SO,²-] [SO]=1.2 x 10 M 1.5 x 105 (0.30) [S0,³-] [SO]=1.7 x 10 M CaSO, requires a smaller concentration of SO, to precipitate, so it will precipitate first. -1 Kap=[Ag¹ [SO]=-1.5 × 10- How much Na SO, solution must be added to initiate the precipitation? Express your answer in liters to two significant figures. 195] ΑΣΦ v-1.2.10-6 X √ √xxx ? X-10" C31 1 L