(15)10. Find the equilibrium pH value if pper ion (Cu2+) concentration in water is 10 mg/L....
Find the equilibrium concentration of aluminum ions in pure water at 25 degree C caused by the dissociation of Al(OH)_3. Express the answer both in units of M and mg/L. Find the equilibrium pH value if copper ion (Cu^2+) concentration in water is 1.2 mg/L. The copper ion is dissolved from Cu(OH)_2. Calculate the equilibrium concentration of dissolved oxygen in mg/L in 10 degree C water (a) at msl (mean sea level), and (b) at 600 m elevation.
1- What is the approximate concentration of free Cu2+ ion at equilibrium when 1.71×10-2 mol copper(II) nitrate is added to 1.00 L of solution that is 1.310 M in NH3. For [Cu(NH3)4]2+, Kf = 2.1×1013. [Cu2+] = ------ M
What is the approximate concentration of free Cu2+ ion at equilibrium when 1.22x102 mol copper(II) nitrate is added to 1.00 L of solution that is 1.210 M in NH3. For [Cu(NH3)4]. Ke-2.1x1013 (Cu?") - Submit Answer Determine ion concentration when separating ions in a mixture. A solution contains 1.58x102 M lead acetate and 1.58x10 ? Mmanganese(II) nitrate. Solid sodium sulfide is added slowly to this mixture. What is the concentration of lead ion when manganese(II)ion begins to precipitate? Solubility product...
please help What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol copperII) nitrate is added to 1.00 L of solution that is 1.380 M in NH3. For [Cu(NH3)4j2, Kf 2.1 1013 [Cu2 м What is the approximate concentration of free Fe2* ion at equilibrium when 1.42x102mol iron(II) nitrate is added to 1.00 L of solution that is 1.38so M in CN. For [Fe(CN)6]4, Kf=1.0x1035 [Fe"]= In the presence of excess OH, the Al*(aq) ion forms...
Find the hydronium ion concentration and pH for the following 1. 2. Calculate the hydronium ion concentration and the pH when 80.0 mL of 0.55 MNH, is mixed with 80.0 mL of 0.55 M HCl (K. = 5.6 x 10-10). Concentration M pH- Phenol (CH-OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(0) = CH.0 (aq) +H3O+ (aq) K= 1.3 x 10-10 If you dissolve 0.593 g of the acid in enough water to...
If the concentration of Mg2+ ion in seawater is 1.29 × 103 mg/L, what OH concentration is required to precipitate Mg(OH)2? Ksp (Mg(OH)2) 5.6x 10-1 OH- concentration must be greater than M.
6. Copper (I) ion undergoes the following disproportionation reaction in water, for which the equilibrium constant is about 106: 2 Cu+ (aq) Cu (s) + Cu2+ (aq) If the copper(I) ion is dissolved in dimethylsulfoxide (DMSO, (CH3)2SO) solvent, however, the equilibrium constant is only about 2. Suggest an explanation based on HSAB Theory (2 pts)
If the concentration of Mg2+ ion in seawater is 1.21x103 mg/L, what OH- concentration is required to precipitate Mg(OH)2 ? Ksp(Mg(OH)2)=5.6x10-12 -OH concentration must be greater than _____ M.
1a.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1b.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1c.) Calculate Ksp = _____ A2BO3 ->2A++ BO32- Molar concentration of A+ = Molar...
The concentration of Cu2+ ion in a sample of spring water is 5.3 ppm. What mass of Cu2+ ion is present in 6.5 L of this pring water, which has a density of 1.00 g/mL? O 2.6 g 0 0.068 g O 0.034 g O 0.34 g