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- 9-The (Ka) value for the reaction of CH3 COOH with NH3 that the PH of the solution-is (6.46) the (Kb=1.75x105) is : a)( 2.1x10 4 b) 2.1x106 c) 1.2 x 106 d) 1.2x10 42) a) What is the [H;O*] of a 2.46 X 10$ M NaOH solution? Is the solution acidic, basic or neutral? (4.06 X 1010 M) b) What is the pH of the solution? (9.391)Write the equilibrium constant expression, Kc, for the following reactions. Indicate also if the equilibrium is homogeneous or heterogeneous. (ONLY 1 AND 2) COMPLETE SOLUTION
- Select from the list below, the Ka value of phosphoric acid, H3PO4. (You will have to do a bit of research to answer this question.) A. 7.5 x 10-3 B. 7.9 x 10-6 C. 6.2 x 10-8 D. 1.8 x 10-5help me pleaseInterconverting pH and hydronium ion concentration Zulema Each row of the table below describes an aqueous solution at about 25 °C. [1,0"] Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for to 2 significant digits, and your entries for pH to 2 decimal places. [1,0] solution PH 11 mol/L 5.6 x 10 mol/L 0.60 B 1.9 x 10 -7 mol/L Explanation Check Terms of Use Privacy 2021 McGraw-Hill Education. All Rights Reserved
- 4. A 850.0 mL sample of HCl(aq) is prepared and has a pH of 1.123. What mass of HCl(g) is dissolved? (answer + units)Ihave some acetic acid that dissociates in water. [CH3COOH] = 0.405 M and [CH3COO]=0.505 M. K3=1.8x10-5. Find the pH=? (3 sig fig)11. A triprotic acid has a concentration of 0.150 M. The Ka1= 1.2x102, Ka2= 3.5x107, ka2= 4.6x10-12. What is the concentration of H3A, H₂A, HA², and what is the pH and hydroxide concentration? (15 points)
- Manganese carbonate (MnCO3) has low solubility in neutral water (8 mg/L), but dissolves completely in water when pH is low. While there is no obvious common ion effect, it does have a distinct solubility relationship. Propose a brief explanation. (2-4 sentences max)Question 15 (1 point) What is the concentration of hydroxide ions in an Al(OH)3 solution with a concentration of 0.166 M? Your Answer: Answer unitsOxalic acid ionizes in two stages in aqueous solution: H2C2O4(aq) + H2O(€ )2H;0* (aq) + HC2O4 (aq) Kal = 5.9 × 10² HC,O, (aq) + H,O(e)2H;0*(aq) + C20?¯(aq) K22 = 6.4 × 10-5 Calculate the equilibrium concentrations of C¿O²¯, HC,O, H,C,O4, and OH- in a 0.10 M solution of sodium oxalate (Na,C¿O4).
