knowing that H₂X react in the water like that H₂₂ X + H₂O <-> H ₂ O ² + H X HX² + 1₂₂0) H₂0² + x²- Find the pit of Solution of the "daughter" H₂ X Pka = 3,2 pka = 5,4
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- Activity 2. Self-ionization of water and pH, pOH, pKw »1. Write the law of mass action for the reaction of self-ionization of water and calculate the concentrations of [H;O*] and [OH]. H,0(1) + H20(1)= H30*(aq) + OH-(aq) Kw = 1.0x10-14 %3D 2 Since working with yery small powers of 10 can be inconvenient, we commonly use the mathematicalWhat is the equilibrium concentration of H3O+ in 0.1564 M HNO2 ? See reaction belowHNO2 + H2O ↔ NO-2 + H3O+ Ka = 4.600x10-43. A solution was prepared by adding 4.95 g sodium acetate (NaC;H;O2) to 250.0 mL of 0.150 M acetic acid (K = 1.75 x 10). Assume negligible volume change. a) What is the pH of the resulting solution? PH: pk2 + log CH3 02) moles saium 4.959 0.06 mol %3D 2cent %3D 82gmu H: -log (1.73x 10) + log 0.24 moles 2cete 250 x 0.15 IL :00375 1000me PH : 4 1.96 O.06 (N2 G Hs0): 0.24m 0.230 L O.0375 : CCHS COOH): 0 15 m Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to it. What is the pH of this new mixture? b)
- How many grams of NaIO (Kb (IO-)=5x10-4 ; MW=213.9 g/mole) must be added to 40.0 ml of 0.1 M HCl to achieve a pH=10.2?Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.If 2 ml of 25 N H2SO4 is transferred to 50 ml volumetric flask and complete to mark with ditilled water, the concentration of acid will be .. M* O 2.5 O 1.5 2 O 0.5 0 1 Non of these
- 3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 1242-14. Calculate the p-value for each of the indicated ions in the following: (a) Na*, Cl, and OH- in a solution that is 0.0235 M in NaCl and 0.0503 M in NaOH. (b) Ht, Cl-, and Zn2+ in a solution that is 0.800 M in HCl and 0.101 M in ZnCl2. K+, OH-, and Fe(CN)- in a solution that is 3.79 X 10-7 M in K,Fe(CN), and 4.12 x 10-7 M (c) in KOH.You may want to reference (Page 834) Section 18.3 while completing this problem. Part A If 130.0 mL of 0.0020 M Na2SO4 (aq) is saturated with CaSO4, how many grams of CaSO4 would be present in the solution? [Hint. Does the usual simplifying assumption hold?] Express your answer using two significant figures. VE ΑΣΦ ? m = 0.43 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining g
- Would the concentration of OH- in the solutions for Runs 2-4 be different if deionized water was used to prepare them instead of aqueous NaCl solution? The OH concentrations were 0.300M, 0.200M, 0.100M, and 0.050M for the runs.2- Suppose a 0.027 M aqueous solution of oxalic and (H₂C₂O) is prepared. Calculate the equilibrium molarity of C₂O You'll find information on the properties of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits. M 0.P XFrom the following choose the most appropriate weak base (when added to its conjugate acid) for making a buffer with pH = 4.50 O (CH3)3N (K, = 6.4 x 105) %3D O CgH5NH2 (K = 3.9 x 1010) O C2H5NH2 (Kg = 5.6 x 104) O HONH2 (K, = 1.1x 108) %3D O NH3 (K5 - 1.8 x 10 5)