Question

1)consider a 1.50 M solution of nitrous acid,HNO2 (ka=6.0*10^-4) what is molarity of H^+? what is...

1)consider a 1.50 M solution of nitrous acid,HNO2 (ka=6.0*10^-4)
what is molarity of H^+?
what is the PH?

2) indiacte speices if its an acid or base?
NH3
+h20
...>
<.... NH4+
+OH
C7H502H
+c6h5nh2
C75O2^-
+C6H5NH3^+

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the pH of a 0.375 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4)...
Calculate the pH of a 0.375 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
For the nitrous acid, HNO2, Ka= 4.0 x 10^-4. Calculate the ph of 0.27 M HNO2
For the nitrous acid, HNO2, Ka= 4.0 x 10^-4. Calculate the ph of 0.27 M HNO2
nitrous acid, HNO2, has a Ka of 7.1 x 10^-4. What are [H3O+], [NO2-], and [OH-]...
nitrous acid, HNO2, has a Ka of 7.1 x 10^-4. What are [H3O+], [NO2-], and [OH-] in 0.60 M HNO2?
What is the pH of a 0.0520 M solution of nitrous acid (HNO2)? (Ka = 4.5...
What is the pH of a 0.0520 M solution of nitrous acid (HNO2)? (Ka = 4.5 x 10-4) (Hint: use ICE and solve the quadratic equation) OR something A LOT simple PLEASE Question options: a) pH = 2.34 b) pH = 2.32 c) pH = 2.30 d) pH = 2.36     
Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2) and 0.178...
Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2) and 0.178 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.
50.0mL of 0.10M HNO2 (nitrous acid, Ka= 4.5x10^-4) is titrated with a 0.10M KOH solution. After...
50.0mL of 0.10M HNO2 (nitrous acid, Ka= 4.5x10^-4) is titrated with a 0.10M KOH solution. After 25.00mL of the KOH solution is added, the pH in the titration flask will be
To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2) and 1.01M potassium...
To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2) and 1.01M potassium nitrite (KNO2) was added 0.625 moles of NaOH (assume no volume change to the solution). What is the final pH of this buffer assuming Ka nitrous acid = 4.00e-4
A 0.540 M Nitrous Acid (HNO2) solution has been mixed with 0.050 M NaCl. What will...
A 0.540 M Nitrous Acid (HNO2) solution has been mixed with 0.050 M NaCl. What will be the hydronium ion concentration of this solution? The activity coefficients for H3O+ and NO2− are 0.86 and 0.80 respectively. The Ka for Nitrous Acid is 5.10000E-4.
Calculate the pH of a solution that is 0.253 M in nitrous acid (HNO2) and 0.111...
Calculate the pH of a solution that is 0.253 M in nitrous acid (HNO2) and 0.111 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 ⋅ 10-4. One of these answers is the correct one. 2.992 11.01 14.36 3.708 4.898
a. Calculate the pH of a 0.538 M aqueous solution of hydrofluoric acid (HF, Ka =...
a. Calculate the pH of a 0.538 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4). b. Calculate the pH of a 0.0242 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).