Q: what is the pH of 1.0 x 108 M solution of H2S04? Ka for the reaction is100 Select one: О а. 8.00 ОБ.…
A: In order to calculate the pH we first write down the given data: Concentration of the acid= 10-8 M.…
Q: Carbonic acid, H,CO, is a diprotic acid with Ka1 = 4.3 × 107 and Ka2 = 5.6 × 1011. What is the pH of…
A: H2CO3 ⇌HCO3− + H+......... ka1= 4.3x10-7 HCO3− ⇌CO3-2 + H+.......... Ka2=5.6x10-11ka1…
Q: a
A: SnCl2 is Lewis acid, when this Lewis acid dissolved in water then this salt will release H+ ion it's…
Q: What is the pH of a 0.350 M solution of HF (Ka = 6.8 × 10⁻⁴)?
A:
Q: What is the pH of the solution prepared by allowing 1.55 g of Na2O to react with 500.0 mL of water?…
A: Reaction: Na2O + H2O→ 2NaOH 1mole Na2O reacts with 1 mole H2O to give 2 moles of NaOH
Q: A 0.495M solution of nitrous acid, HNO2, has a pH of 1.83. Calculate the value of Ka for nitrous…
A:
Q: The pH of a 0.15-M solution of HSO4− is 1.43. Determine Ka for HSO4− from these data.
A: Given, initial concentration of HSO4− = 0.15 M pH = 1.43 We know that, pH is the negative…
Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00298 M…
A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid
Q: Calculate the molar concentration of OH− ions in a 0.069 M solution of ethylamine (C2H5NH2;…
A:
Q: Calculate the pH of a solution that is 0.410 M in HOCI and 0.050 M in NaOCI. [Ka(HOCI) = 3.2 x 10-8)…
A: Concentration of HOCl=0.410M Concentration of NaOCl=0.050M Ka(HOCl)=3.2 × 10^-8
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: Calculate the pH of a 3.12×10-3 M solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.
A:
Q: Calculate the pH of a solution containing 0.3 M HCOOH and 0.1 M HCOO (pKa of HCOOH = 3.76)
A: Concentration of HCOOH (Acid) = 0.3 M Concentration of HCOO- (conjugate base of acid) = 0.1 M pKa…
Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)?
A: Given concentration of CH3COOH = 1.75 × 10-5
Q: Find the pH of a 0.2 M solution of H2SO3
A: Given, The pH of a 0.2 M solution of H2SO3 is:
Q: a general chemistry student measured the pH of a 0.510 M aqueous solution of nitrous acid to be…
A: Here we are required to find the dissociation constant for weak acid nitrous acid
Q: What is the pH of a 0.390 M solution of HF (Ka = 6.8 × 10⁻⁴)?
A:
Q: Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed…
A:
Q: Calculate the pH of a 0.010-M solution of iodic acid (HIO3, Ka = 0.17).
A: Molarity of Solution = 0.010M Ka of Acid = 0.17 We have to find the pH of the solution of iodic…
Q: Calculate the pH and [S2−] in a 0.10-M H2S solution. Assume ka1= 1.0 × 10−7; ka2= 1.0 × 10−19.
A: Answer:- This question is answered by using the simple concept of calculation of pH of a weak acid…
Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56
A: The concept used here is based on the acid dissociation constant of an acid which is used for…
Q: Calculate the pH of 2.5 M CH2ClCOOH(aq) given that its Ka = 0.0014.
A:
Q: Calculate the pH of a 0.100 M NaHCO3 solution.
A: The pH of a given solution can be defined as the measure of its basicity or acidity. More the pH…
Q: What is the pH of a solution that is 0.100 M in NaHCO3?
A: Given, 0.100 M in NaHCO3
Q: Calculate the pH of a solution that is 0.052 M in HCl and 0.020 in HClO4
A: Given that, The concentration of the solution in HCl = 0.052 M And the concentration of the…
Q: Calculate the pH of a 0.31 M sodium formate solution (HCOONa). Kb for HCOO− = 5.9 × 10−11
A: Given :- [HCOONa] = 0.31 M Kb for HCOO- = 5.9 × 10−11 To calculate :- pH of solution
Q: 3. How is K, obtained by the half-neutralization method?
A: Since you have posted multiple questions, we will solve the first question. Please post rest of the…
Q: What is the pH of a 0.028 M solution of pyridine? The pKa for the pyridinium ion is 5.20. a)7.00…
A: pH of solution is determined by taking negative logarithm of hydronium ion concentration.…
Q: Calculate [H3O+] and pH for a 0.317 M solution of HF; Ka = 6.8 × 10−4.
A: Given, Concentration of HF (C) = 0.317 M Dissociation constant of HF , Ka = 6.8×10-4 [H3O+] = ? pH =…
Q: At 25°C, the Henry’s law constant for carbon dioxide dissolved in water is 1.8 × 103 atm. Calculate…
A: According to Henry's law,the vapor pressure of the substance dissolved in the solution is directly…
Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.
A: Concentration of Al ion = 0.064 M
Q: 2. Calculate the pH of a 0.200 M solution of H2SO4. Ka2 for H2SO4 is 1.2 x 102. (Since Kaz is high,…
A: Step -1 we know that PH = -log(H+) H2SO4 - gives two H+ ions in dissociation condition. So, 2 x…
Q: What is [H3O+] of a softdrink that has a pH of 3.400?
A: Given-> pH = 3.400
Q: Calculate the pH of a 0.20 M solution of NH4NO3. (Kb(NH3) = 1.8 x 10)
A: Salt of Weak base and Strong acid pH = 7 - 1/2 ( pKb - logC )
Q: Calculate the pH of a 0.10 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…
A:
Q: Calculate the pH of a of 0.100M KBRO solution. Ka for hypobromous acid, HBRO, is 2.0 x 10 6- 10.85…
A: Given: The concentration of the KBrO3 solution = 0.100 M The Ka for HBrO3 = 2.0 × 10-9 We have to…
Q: Calculate the pH of a solution resulting from the addition of 50.0 mL of 0.30M HNO3 to 50.0 mL of…
A: Nitric acid which is a strong acid on undergoing a reaction with ammonia will form a salt of…
Q: B. Calculate the PH and to YOH FOR 9.209 M Solution Cr (₂(04),
A:
Q: 22:b) Solution A has a PH = 8.94 and Solution B has a [OH] = 4.5 x 10+ M. Which solution is more…
A: Here is the solution
Q: Calculate the pH of a 7.8 * 10 ^ - 3 M solution of RbOH
A:
Q: What volume of 2.036 mol L-1 solution of LIOH is required to make 7.80 L of a solution with a pH =…
A: Given :- Initial concentration of LiOH solution = 2.036 mol.L-1 pH of final solution = 12.80…
Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…
A: Since the Ka1 of H2CO3 is >> Ka2 of H2CO3 Hence we can assume only the first dissociation of…
Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00789 M…
A:
Q: Calculate the pH of a solution that has a 0.0025 M [H3O] +
A: PH= -log[ H3O +] NEGATIVE LOHARITHAM OF HYDRONIUM ION CONCENTRATION
Q: Determine the pH of the solution resulting from mixing a solution of 154 mL of HNO2 (Ka = 5.62e –…
A:
Q: How many grams of H2SO4 could be neutralized by 16.2 mL of 0.370 M KOH?
A: Given that : The volume of KOH = 16.2 mL The molarity of KOH = 0.370 M We have to calculate the mass…
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 a solution of 0.25M Nacio(ag). The Ka of HCIO is 2.9 x 108.
A: NaClO is a salt of weak acid HClO. It has pH greater than 7 as it is base.
Q: Calculate the pH of a solution that is 0.70 M in HF (Ka =7.2 x 104) and 0.66 M in NaF. а. 3.40 O…
A:
Answer number 3 only
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
- 1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?The temperature for each solution is carried out at approximately 297 K where Kw=1.00 x 10-14- a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? Express the pH numerically to two decimal places. b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution? Express the pH numerically to two decimal places.An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. What is the effect of adding 0.50 mol CH3CO2–(aq) to this solution? 1.The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2.Some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2–(aq) and increasing the pH.3.Some CH3CO2–(aq) will react with H3O+, increasing the concentration of CH3CO2H(aq) and reestablishing the solution equilibrium. b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3
- Calculate the pH and [H3O+] of a soln that is 0.050 M in HC2H3O2and 0.10 M in NaC2H3O2. What happens when 1.0 x 10-3 mol of HClare added to this soln?Ka HC2H3O2 = 1.80 x 10-51. Write a chemical equation for the dissociation of the hypochlorite ion, ClO-1, in water to make a basic solution. 2. The Ka for benzoic acid (HC7H5O2), is 6.5 x 10-5. Calcuklate pH of a 0.10 M benzoic acid solution. 3. Calculate the pH of a 0.24 M solution of weak base A-1 that has a Kb of 2.5 x 10-6.An organic acid(HA) has a molecular weight of 100. g mol^-1, a Kow=5.6 and a Ka=2.7x10^-2. If originally 2.0g of the acid is dissolved in 100mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100mL of water, what will be the pH of the water? (consider the equilibrium processes to be sequential and unrelated chemically)
- Calculate the pH of the following solutions. (1)Tap water after boiling (2) 0.0010 M NaOH aqueous solution (3) 10-9 M NaOH aqueous solution. (4) 0.20 M HAc (acetic acid, Ka(HAc) = 1.8 x10-5 ) (5) 0.20 M NaAc (sodium acetate). (6) 0.8203 g NaAc (FW=82.03 g/mol) was fully dissolved into 100.00 mL of 0.050 M HAc solution.The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10−14. a) 0.60 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution? b) 0.45 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 4.5 L of solution. What is the pH of this solution?Potassium hydroxide (KOH) is a strong base. Dissociation of potassium hydroxide follows the reaction equation given. KOH(s) --H20--> K+(aq) OH-(aq) a) Write down the reaction equation for a neutralization reaction where potassium hydroxide (KOH) reacts with sulphuric acid (H2SO4) producing potassium sulphate (K2SO4) and water (H2O). Balance if needed! b) Calculate pH for the solution where 0,2 mol of KOH is dissolved into water so that the total volume of the solution is 0,5 L.
- 2. A 0.0560-g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H+,CH3COO ,and CH3COOH at equilibrium. (Ka for acetic acid is 1.8 x 10-5)3. The pH of an acid solution is 6.20. Calculate the Ka for the acid. The initial acid concentration is 0.010 M. 4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium? 5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. Calculate the percent ionization of Ammonium hydroxide, NH4OH at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain…The Kb of C6H5NH3+ is 3.98x10-10 What is its Ka? What is the [H3O+] concentration in a solution that is 4.25x10^-4 M C6H5NH3+? What are the pH and pOH of the solution, respectively? What is the molar solubility of Ag2CO3 in pure water, given that its Ksp= 8.10x10-12?The Ka of an acid is known to be 1.51 X 10^-5. A solution is made by adding 0.279 mol of the acid to enough water to make the final volume 1.30 L. a. what is the equilibrium concentration of H_3O+ b. what is the equilibrium pH of the solution c. what is the equilibrium concentration of the conjugate base d. what is the equilibruim concentration of the acid e. what is the % dissociation of the acid