Calculate the pH of a 3.5 x 103 M HNO3 solution. Multiple Cholice 2.46 3.46

Q: The organic acid RCOOH has a pk = 4.08. What is the pH of a 0.50 M aqueous solution of this acid?…

A: Given: pKa of organic acid = 4.08 Concentration of organic acid = 0.50 M

Q: Calculate the pH value of a 0.20 M solution of NH4Cl (Kb (NH3)= 1.79 × 10 -5).

A: Given, Concentration of NH4Cl = 0.20 M  Base dissociation constant for NH3 kb = 1.79 x 10-5 PH of…

Q: Calculate the pH of a solution that contains 3.9 x 104 M H3O* at 25°C. 4.59 3.41 10.59 9.41 0.59

A: Given, Concentration of H3O+ ion = [H3O+] = 3.9 × 10-4 M Temperature (T) = 25°C pH of the solution =…

Q: Calculate the pH of a 0.40 M solution of(C2H5)2NH (Kb=1.3x10^-3)

A:

Q: Calculate the hydronium ion concentration of a 0.1000M NaHCO3 solution. [Ka1 = 4.4 x 107,Ka2 = 4.7 x…

A:

Q: Calculate the pH of a 0.6 M solution of Na,S. For H2S: Ka1 = 9.1x10 Ka2 = 1.2x10 15 a. 7.18 b. 14.35…

A: NOTE: the answer is not matching with the exact solution out of the options given. so,  I have…

Q: Calculate the pH of a 0.053 M NaF solution. (Ka for HF = 7.1 x 10−4.)

A: NaF is a salt of strong base (NaOH) and weak acid (HF)

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.100 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Ka = 4.5*10^-4 (given) pKa = – log [ Ka ] = – log(4.5*10^-4) = 3.347 Now, By using Henderson…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.200 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: By using Henderson Hasselbalch equation the pH of the buffer solution is determined by using the…

Q: Chemistry Like aqueous solutions of Fe3+, bismuth ions (Bi3+) form acidic solutions with a pKa =…

A:

Q: What is the pH of a 0.310 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)

A: Since aniline is a weak base. Hence it will dissociate as  C₆H₅NH₂ (aq) + H2O (l) ------->…

Q: The pH of a 0.12 M HNO3 solution is -1.22 -0.92 0.92 1.22

A: Given concentration of HNO3 = 0.12 M

Q: Determine the pH of each solution. 0.23 M KCHO2 (Ka(HCHO2)=1.8×10−4) 0.18 M CH3NH3I…

A: We need to determine the pH of the each solutions below :1.  0.23 M KCHO2      Ka of HCHO2=1.8×10-4…

Q: Calculate the pH of a 0.30 M solution of NH 4Cl (Kb for NH 3 = 1.8 x 10 -5). a. 11.67 b.…

A: NH4Cl is the salt weak base NH4OH and a strong acid HCl therefore hydrolysis constant Kh will be…

Q: 3. Calculate pH of 0.03 M solution of potassium hydrogen phthalate (KHP). pKr= 2.95, pK=5.41

A: According to the pH scales there are three types of solution are present neutral, acidic and basic…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.170 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: pH of a solution is defined as the negative logarithm of H3O+ ion concentration. Here the given…

Q: A solution of HCIO4 was found to have a pH of 0.14. What is the concentration of HCIO4? a. 7.2 x…

A: HClO4 solution has a pH of 0.14 .We have to calculate the concentration of HClO4 solution .

Q: Calculate the pH of a solution containing 0.03 M NaH2VO4, and 0.05 M Na2HVO4 (Ka1- 1.11.10-2, Ka2 =…

A: Please be noted that the formula of the compound is NaHVO4- but not Na2HVO4.   pH=- log H+ For a…

Q: The pH of 0.65 M aqueous solution of a weak base (monoprotic) is 10.24. Determine the pKp of this…

A:

Q: What will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2…

A: Given,  Molar concentration of weak acid, NaH2PO4 or H2PO4- = [H2PO4-] = 0.200 M Molar concentration…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.140 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Given : Concentration of HNO2 = 0.300 M Concentration of NaNO2 = 0.140 M And Ka of HNO2 = 4.5 X 10-4…

Q: 5.796

A: Kb = 10-pKb  Kb = 10-5.796 Kb = 1.6 • 10^-6

Q: Barium fluoride (BaF2) has Ksp = 1.8 x 107. VWhat is the maximum fluoride ion concentration possible…

A: Given: Ksp of BaF2 = 1.8 x 10-7 Concentration of Ba2+ = [Ba2+] = 5.0 x 10-4 M

Q: Calculate the concentration of free Ca²⁺ in a solution of 0.10 M CaY²⁻ at pH 10.00. (K= 5.0 × 10¹⁰)

A:

Q: What is the pH of a solution that is 0.063 M in HA and also 0.023 Min NaA? (Ka = 4.1 × 10- O. 5.46…

A: Given: The concentration of HA is 0.063 M The concentration of NaA is 0.023 M The Ka value is 4.1 x…

Q: Calculate the pH of a 0.299 M NH, solution. NH, has a Kp = 1.8 × 10-5. pH =

A: pH =11.366

Q: What is the pH of a solution of 0.06 M of H2CO3, pKa1 = 6.4 and pKa2= 10.3?

A: We will calculate pH

Q: Calculate the pH of 0.1 M from sodium acetate CH3CO2Na and hydrolysis percent ? if you know Ka =…

A: Reaction of sodium acetate in water can be written as, CH3COONa + H2O →CH3COOH +Na+ + OH-

Q: concentration 100 times greater than a soluti on with a pi of 4? A S B 2 C. 3 D. 6

A: Solution- pH= -log[H]4=-log [H+]H+= antilog[-4]H+=10-4

Q: Calculate the pH of a solution containing 0.03 M NaH2VO4 and 0.05 M Na2HVO4. (Ka1 = 1.11×10-2, Ka2 =…

A:

Q: 6. What is the pH of 0.5 M nitrous acid (HNO2) ( Ka = 4.5 x 10-4) %3D www

A: Find the pH of HNO2 having 0.5 molarity  Given ka = 4.5 x 10-4

Q: Calculate the pH of a 0.654 M solution of an acid with Ka = 2.33 x 10-5.

A:

Q: Calculate the pH of a 0.325 M solution of a weak base whose conjugate acid has a pka-5.155.

A:

Q: Barium fluoride (BaF2) has Ksp = 1.8 x 107. What is the maximum fluoride ion concentration possible…

A: The solubility product constant (Ksp) describes the dissolution of solute in a solution, which is…

Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?

A:

Q: 8 g of potassium chloride is dissolved in a quart of distilled water. Calculate the pH value of the…

A: Here 8 gram of KOH is dissolved in a quart of distilled water. We have to calculate the pH of…

Q: What is the pH of a solution that is 0.03M in picric acid and 0.1M in sodium picrate. pka=0.38 O a.…

A: The solution is mixed by adding picric acid to sodium picrate. Sodium picrate is made by adding…

Q: What is the pH of a solution that is 0.048 M in HA and also 0.042 M in NaA? (Ka = 4.1 x 10-6) 6.82…

A: Given, Ka for NaA = 4.1 x 10-6  PH = ?

Q: Calculate the concentration of H2SO3 in a 0.510 MM solution of H2SO3 Ka1=1.6×10−2 and Ka2=6.4×10−8).

A: NOTE: In question, you have mentioned 0.510 MM instead of 0.510 M. Hence I'm correcting it and…

Q: What is the pH of a 0.64 M solution of NH3 (Kb = 1.2 × 10-5)?

A:

Q: Calculate the pH of 5.40 g of K2SO3 that has been completed with 500 mL H2O (pKa1= 1.85 and pKa2 =…

A: Weight of K2SO3 = 5.4 g Mol mass of K2SO3 = 158.26 g/mol Volume of H20 = 500 ml Calculation is done…

Q: Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2) and 0.290 M in potassium…

A:

Q: Calculate the pH of a 0.20 M solution of NH4NO3 Kb(NH3) = 1.8x10^-5 Thank you :)

A: A pH scale is a scale that is used to determine the acidic and basic nature of a solution. If the pH…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.210 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: BUFFER SOLUTION It is a solution of weak acid or base with their corresponding conjugate base or…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.220 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

A: Henderson Hasselbalch equation. We can use pOH = pKb + log [salt] / [base]

Q: calculate the PH and the POH FOR solution OF HNO₂ a Ki FOR AM₂ = 5₁1x10-7 .00841

A: 0.0084 M solution of HNO2 has a Ki of 5.1 × 10-4 .We have to calculate the value of pH and pOH .

Q: 3. Calculate the concentration of all species (including H3O* and OH) in a 0.500 M solution of H;SO3…

A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…

Q: Calculate the pH of 0.0470 M LiBrO. Ka of HBrO = 2.8 x 10-9

A: The molarity of LiBrO solution is = 0.0470 M The dissociation constant of the weak acid HBrO is =…

Q: Calculate the hydronium ion concentration of 0.1 M Na2PO4.ka1 =7.11 x10^-3;ka2=6.32 x 10^-8;ka3= 4.5…

A: Given Calculate the hydronium ion concentration of 0.1 M Na2PO4.ka1 =7.11 x10^-3;ka2=6.32 x…

Q: What is the pH of a 0.35 M solution of methylamine (CH3NH2, Kb 4.4 at 25°C? O a. 5.55 b. 12.09 O c.…

A: We will. Calculate pH