KOH(s) was added to 1.0 L of HNO3(aq) 0.30 M. Calculate [H3O+] in the solution after the addition of 0.87 mol of KOH(s).
KOH(s) was added to 1.0 L of HNO3(aq) 0.30 M. Calculate [H3O+] in the solution after...
NaOH (s) was added to 1.0L of HClO4 (aq) 0.49 M. a) Calculate [H3O+] in the solution after the addition on 0.11 mol of NaOH (s) b) Calculate [H3O+] in the solution after the addition of 0.84 mol of NaOH (s)
A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at 0.010 M, was saturated with H2S(g) at room temperature. Assume that the pH of the solution remains constant and that the [H2S]sat = 0.10 M. The Ksp for MnS9S) is 2.5 x 10-13 , Ksp for CdS(s) is 8.0 x 10 -27 and Ksp for FeS(s) is 6.3 x10-18 . For H2S:Ka1=1.3 x 10-7. Ka2=8.5 x 10-14. Calculate the equilibrium concentrations of Mn2+(aq),Cd2+(aq), and...
In a 1.0× 10–6 M solution of HNO3(aq) at 25 °C, identify the relative molar amounts of these species. HNO3, OH^-,H3O^+,NO3^-,H2O
68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution. The end point is reached after 25 m/L of KOH solution is added. what is the molarity of the HNO3 solution ? 1 р . HNO3 + KOH --> KNO3 + H20 68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution. The endpoint is reached after 25.0 mL of KOH solution is added. What is the molarity...
acids: 0.5 mol of NaOH is added to 1.0 L of a 0.3 M HCN solution. bases: 0 o other: 0 0.1 mol of HNO3 is added to 1.0 L of a solution that is 0.4 M in both HCN and NaCN. O acids: 0 O bases: 0 o other: Explanation Check
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.
In a 1.0� 10�6 M solution of HNO3(aq) at 25 �C, identify the relative molar amounts of these species from Most to Least: H2O HNO3 H3O NO3 OH
C) 3400 D ) 2000 Q10: 1.0 L of 1 M NaOH(aq) and 1.0 L of 1 M HNO3(aq), both initially at 25.0 °C, were mixed in a calorimeter. The temperature of the solution increased to 31.1°C. Calculate the enthalpy of neutralization in KJ/mol)? Assume that the specific heat capacity of all solutions is 4.184 J/gºC, the density of all solution is 1.00 g/ml and that the calorimeter doesn't absorb any heat. A) -80.1 kJ/mol B) - 77.8 kJ/mol C)...
A 36.80-mL sample of 0.250 M HNO3 solution is titrated with 0.221 M KOH. Calculate the pH of the solution a before the addition of KOH pH= b after the addition of 6.45 mL KOH pH Cafter the addition of 13.20 mL KOH pH dafter the addition of 26.74 mL KOH pH e after the addition of 38.63 mL KOH pH f after the addition of 42.23 mL KOH pH К, - 1.8 х10-5 К 7.4 х 10-5 К, 5.0...
Calculate [H3O+] for a 3.44×10−3 M HBr solution. Calculate [H3O+] for a 1.00×10−2 M KOH solution.