Determine the pH of an HNO2 solution of each of the following concentrations.
a. 0.510 M
b. 0.110 M
c. 1.30×10−2 M
Determine the pH of an HNO2 solution of each of the following concentrations. a. 0.510 M...
Determine the pH of an HNO2 solution of each of the following concentrations. A) 0.550M B) 0.100M C) 1.2x10^-2 M D) In which cases can you not make the simplifying assumption that x is small? only in (b) only in (a) in (b) and (c) in (a) and (b) PS: Express your answer to two decimal places
Determine the pH of an HF solution of each of the following concentrations. HELP PLEASE. Determine the pH of an HF solution of each of the following concentrations. 5.30x10^-2 Express your answer to two decimal places. Part C 2.00 x 10^-2 M Express your answer to two decimal places.
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M
Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8×10−4.) Part A 0.280 M Express your answer to two decimal places. Part B 4.70×10−2 M Express your answer to two decimal places. Part C 2.70×10−2 M Express your answer to two decimal places. Part D In which cases can you not make the simplifying assumption that x is...
Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that is small? (K, for HF is 6.8 x 10 ) Part A 0.260 M Express your answer to two decimal places. VALD + O 21 ? pH = Submit Request Answer Part B 5.00x10-2M Express your answer to two decimal places. 30 AL * O 31 ? pH = Submit Request Answer Part C 2.00x10-2M Express...
A 1.0-L buffer solution is 0.130 M in HNO2 and 0.180 M in NaNO2. Part A) Determine the concentrations of HNO2 and NO−2 after addition of 1.2 g HCl. Part B) Determine the concentrations of HNO2 and NO−2 after addition of 1.2 g NaOH. Part C) Determine the concentrations of HNO2 and NO−2 after addition of 1.2 g HI.
A 1.0-L buffer solution is 0.135 M in HNO2 and 0.145 M in NaNO2. Part A Determine the concentrations of HNO2 and NaNO2 after addition of 1.3 g HCl. Part B Determine the concentrations of HNO2 and NaNO2 after addition of 1.3 g NaOH Part C Determine the concentrations of HNO2 and NaNO2 after addition of 1.3 g HI.
1) Calculate the pH of a solution that is 1.00 M HNO2 and 1.00 M NaNo2? 2) Calculate the pH after .10 mol NaOh is added to 1.00 L of the solution ?
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
A 1.0 L buffer solution is 0.125 M in HNO2 and 0.195 M in NaNO2. 1. Determine the concentrations of HNO2 and NaNO2 after addition of 1.7 g HCl 2. Determine the concentrations of HNO2 and NaNO2 after addition of 1.7 g NaOH 3. Determine the concentrations of HNO2 and NaNO2 after addition of 1.7 g HI