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- 6-19. A solution contains 0.050 0 M Ca?+ and 0.030 0 M Ag+. Can 99% of Ca?+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate? 24What is the pH of a saturated solution of Ca(OH)₂? Ca(OH)₂ (s) Ca²+ (aq) + 2 OH- (aq) село N O +25 25 initial -§. pH of Hydroxides - Example ех сего +s S Ksp= [Ca²+] [OH-]²= (5)(25)²=453 5= 33.7x² 3.7 хо S (OH) = 25 = 0.019487 M = 0.009713 M Ksp = 3.7 x 10-6 [++] = 10²] -14 pH=12.29 -= 5-1316x180-13 [он) pH = -log (H+) =-loğl pH = 12.28977-43. Supply the missing data in the table below. Molar Analytical Concentration, c- (ct = Cha + cx-) pH (A"] Acid (HA] Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 0.145 0.221 Hydrogen cyanide Sulfamic 0.250 1.20
- 6-39. An acidic solution containing 0.010 M Lat is treated with NaOH until La(OH), precipitates. At what pH does this occur?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 mathematicalry-144 021 / Natural Sciences Chemistry And Polymer Science Chemie - Chemistry - 144 Praktika 2 Verslag Watter komponent van die vo oplossing het tydens Experim tydens die byvoeging van die During Experiment 2, what component of the prepared buffer solution reacted during the addition of the strong base, NAOH? Select one or more: The conjugated base of the weak acid. Die gekonjugeerde basis van die swak suur. The acetic acid molecules. Die asynsuur molekules. No reaction takes place as buffers are able to resist any changes in solution. Geen reaksie vind plaas nie want buffers kan veranderinge weerstaan in oplossing. The acetate ions. Die asetaat ione. The conjugated acid of the weak base. Die gekonjugeerde suur van die swak basis.
- Questions 30-35 refer to the same weak acid/strong base (WA/SB) titration. Prior to the beginning of the titration, there were 0.0090 moles of hypobromous acid present in the flask. The Ką of hypobromous acid is 2.8 x 10-9. (Q30) A 30.00 mL solution of 0.300 M hypobromous acid (HBRO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LIOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)?Determine concentration of OH- in a 0.724 M solution of BrO- (Kb = 4.0 × 10-6). 1 2 NEXT > Based on the given values, set up ICE table in order to determine the unknown. BrO (aq) H:O(1) OH-(aq) HBRO(aq) + + Initial (M) Change (M) Equilibrium (M) 5 RESET 0.724 4.0 x 10-6 0.362 +x -X +2x -2x 0.724 + x 0.724 - x 0.724 + 2x 0.724 - 2x 4.0 x 106 + x 4.0 x 106 - x 4.0 x 10-8 + 2x 4.0 × 10-8 - 2xthank you
- B. Molar Concentration of an Acid Solution Acid type, HA or H,A: HA Unknown No. Balanced equation for neutralization of acid with NaOH. NaOH + HCI = NaCI + Sample 1 Sample 2 Sample 3 1. Volume of acid solution (mL) 25.0 25.0 25.0 2. Buret reading of NaOH, initial (mL) 0.00 0.00 0.00 3. Buret reading of NaOH, final (mL) 26.3 26.0 26.8 26.3 26.0 0.148 4. Volume of NaOH dispensed (mL) 26.8 5. Molar concentration of NAOH (mol/L), Part A 6. Moles of NaOH dispensed (mol) 7. Molar concentration of acid solution (mol/L) 8. Average molar concentration of acid solution (mol/L) Data Analysis, B 9. Standard deviation of molar concentration Data Analysis, C 10. Relative standard deviation of molar concentration (%RSD) Data Analysis, D7-43. Supply the missing data in the table below. Molar Analytical Concentration, c- Acid (Ct = CHa + Ca-) pH (HA] [A^] Lactic 0.120 0.640 Iodic 0.200 0.765 Butanoic 5.00 0.0644 Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 Hydrogen cyanide Sulfamic 0.145 0.221 0.250 1.20If you could help with the below pre-lab questions please. PRELABORATORY ASSIGNMENT Define the term "salt.' The solubility of AgCl(s) in water is 1.3 x 10-5 M. Calculate its Ksp. The solubility of CsF2(s) in water is 2.1 x 10-4 M. Calculate its Ksp. The of Pb(OH)2 is 4 x 10-15. Calculate the molar solubility of this compound.