6. What is [H3O+] in a solution of 0.075M HNO2 and 0.030M NaNO, Ka of HNO2...
1.) a buffer solution is 0.453 M im HNO2 and 0.339 M in NaNO2. If Ka for HNO2 is 4.5x10^-4, what is the pH of this buffer solution? pH = ???? 2.) A buffer solution is 0.373 M in H2C2O4 and 0.303 M in KHC2O4. If Ka1 for H2C2O4 is 5.9x10^-2, what is the pH of this buffer solution? pH = ???? 3.) a buffer solution is 0.333 M in KH2PO4 and 0.248 M in K2HPO4. If Ka for H2PO4^-...
Nitrous acid, HNO2, has a Ka of 7.1 × 10−4. What are [H3O+], [NO2−], and [OH−] in 0.54 M HNO2?
What would be the pH of a buffer that contains 0.987 grams of Nitrous acid (HNO2) and 1.242 grams of sodium Nitrite (NaNO2), in 250ml of solution?(Ka of Nitrous acid = 4.5X10-4)
What is the pH of a 0.35 M solution of NO2-? (Ka of HNO2 = 4.0 x 10-4) 7.32 8.47 5.53 9.86 4.16
What is the pH of a 0.043 M solution of nitrous acid, HNO2? Ka = 4.6 x 10-4
What is the pH of a solution prepared to 0.040 M NaNO2. Ka HNO2 = 7.1 x 10-4
What is the pH of a 1.00 molar solution of NaNO2(aq)? The Ka for HNO2 is 7.0*10^-4 (Please include how you solved the problem. Thanks!)
What is the expected pH of a 0.665M solution of nitrous acid in water? Ka(HNO2) = 4.573x10-4 (pH is a unitless quantity)
Given 0.114 M HNO2 in water with a Ka for that acid of 4.6x104, what is the molarity of NO2 "present in that solution? 7.2x10-3 3.2x10-2 O 5.2x10-5 O 1.6x10-6 O 1.1x10-4
What is the pH of a 0.50 M NO2- solution. The Ka of HNO2 is 4.5 x 10-4. a) 7.54 b) 8.52 c) 8.30 d) 7.76 e) 8.04