Calculate the Ka of a 0.400 M acid solution with [H30*]= 1.4x 10 4M O 1.40 x 106 O 1.40 x 10 5 O 4.90 x 10 7 O 4.0 x 107 O 4.90 x 10 8 O 4.0 x 101

Q: Calculate the pH of a 0.150M solution of aniline, C₆H₅NH₂ ka=4.0E-10

A: Answer:Negative of logarithm of OH- ion concentration is equal to pOH, so,Also,

Q: What is the pH and % ionization of a 0.25 M aqueous solution of hydrazine? Kb = 1.3 x 10-6

A: The objective of this question is to calculate the pH and percent ionization of a 0.25 M aqueous…

Q: 2. Calculate the pH at 25 °C of a solution that is 0.3 M in NaH2AsO4 at 25 °C (Kal =5.8 x 10, Ka2 =…

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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: [Ka1 = 5.4 x 10-6; Ka2 = 5.8 x 10-10 %3D OA.0.10 M OB. 5.8 x 10-6 M OC21x 10-5 M OD.5.4 x 10-10M O…

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Q: What is the pH of a 0.030 M solution of oxalic acid? Ka for oxalic acid is 5.9 x 10-2.

A: pH of weak acid can be calculated by considering its Ka value.

Q: Calculate the concentrations of ALL the ions present in a 0.0300M solution of carbonic acid (H2CO3…

A: H2CO3 is a weak acid. It is form from the reaction of CO2 with water. Given data:  Ka1 = 4.2×10-7…

Q: What is the percent of the unprotonated form of ammonia (K₂ NH3 = 1.74 x 10-5) in a solution at pH…

A: The objective of this question is to find the percentage of the unprotonated form of ammonia in a…

Q: Calculate the pH of a 0.018M H2SO4 solution that has a Ka1=strong and Ka2=1.2•10-2

A:

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: What is the pH of a 0.15 M HOBr solution (Ka = 2.3 x 10-9)?

A: Given Data : 1. Ka = 2.3 x 10-9  2. Concentration C = 0.15 M

Q: calculate the pH of a 3.8 M solution of aniline (Ka (aniline salt) = 2.33 x 10-5)

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Q: Calculate the pH for 0.0150 M H₂CrO solution. For H₂CrO, Ka₁ is very large and Ka₂ is 3.10 x 10-³.

A: Given , Concentration of H2CrO4 =0.0150 M

Q: the diprotic weak acid H₂A, K₁1 = 3.3 x 10 and K₁2 = 7.7 x 10⁹. hat is the pH of a 0.0600 M solution…

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Q: α A solution is prepared at 25 °C that is initially 0.90M in chloroacetic acid (HCH2CICO2), a weak…

A: Thank you,Please rate my response.

Q: Calculate the PH and the POH for a .66 moles solution of NH3  Ki for NH3 = 1.9 x 10-5

A: To calculate the pH and pOH of the solution, we need to first determine the concentration of…

Q: The equilibrium                         2 H2O(l)  ⇆  H3O+(aq) + OH−(aq)  Kc = 1x10−14 occurs in…

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Q: The pH of a 0.063-M solution of hypobromous acid (HODI but usually written Dr) is 4.92. Calculate…

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Q: What is the pH of a 0.350 M solution of lithium citrate? (K₂ Citric Acid = 7.4 x 10-4)

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Q: What is the equilibrium concentration of [H3O+] in a 0.20 M aqueous solution of HNO3? 10-7 M 0.4 M…

A: Given: Concentration of  HNO3 solution = 0.20M

Q: 4. Sodium hypochlorite (NaCIO) is often found in household bleach. What is the pH of a 0.740 M…

A: We have to predict the pH of solution .

Q: Calculate the pH of a 0.025 M solution of propanoic acid (K, = 1.3 x 10-5). 7.48 0.025 O 5.6 x 104…

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Q: Calculate the expected pH of a solution of 30.0 mL of 1.50 M nitrous acid mixed with 19.6 mL of…

A: Given,Molarity of HNO2 = 1.50 MVolume of HNO2 = 30.0 mLMolarity of NaOH = 0.968 MVolume of NaOH =…

Q: Calculate the pH of 0.30 M NaOH solution ?   Kw = 1.0 x 10-14

A: pH is defined as the concentration of hydronium ion in the solution

Q: A solution of 2.5 M weak acid is 1.52% ionized. What is the Ka value of this acid? cof O 32x 104 O…

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Q: -3 Calculate the pH of a 3.6 x 10-M solution of H2SO4 (Ka, = 1.2 x 10-2). pH =

A:

Q: Calculate the pH of 3.5M citric acid solution at 25⁰C when the Ka is 7.1 x 10-4.

A: Give information: Concentration of solution = 3.5 M Ka is 7.1 x 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 =…

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Q: [OH"]

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Q: . Calculate the pH of a 0.150 M solution of carbonic acid (H₂CO3)? Kal = 4.5 x 10 7 Ka2 = 4.7 x 10…

A: pH is equal to negative logarithmic of hydrogen ion concentration

Q: Calculate the pH of Ka for HCHO₂ is 1.8 × 10 a 0.10 M Na CHO₂ solution. -4

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Q: What is the concentration of fluoride ions (F) in a solution containing 0.050 M HCI and 0.085 M HF…

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Q: Calculate the [H+] concentrate if pOH = 5.35

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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: 3. Calculate the pH of a 0.400 M KC2H3O2 (Ka for HC2H3O2 is 1.8 x 10-5)

A: In this question we have to tell the PH of the solution.

Q: What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7…

A: The H3O+ concentration for the weak acid is determined given below:

Q: What is the pH of rainwater in equilibrium with 0.531 ppm SO2 (KH = 1.0 M-atm 1) when sulfurous acid…

A:

Q: What is the pH of a 0.35 M solution of hydrofluoric acid with a K, of 6.6 x 104? 3.23 O 1.82 O 5.47…

A: Given: Concentration of HF acid = 0.35 M Ka of HF = 6.6×10-4

Q: Calculate the pH of a 0.383 M NH, solution. NH, has a Kp 1.8 x 10-5. pH

A: NH3 is a weak base and since Kb value is very less so it is assumed that reaction proceeds very less…

Q: 5. Complete table. a of the Solution Relevant Values [H30*] pH pOH [OH¯] solute 0.014 Μ ΗΝΟ3 N/A…

A: The strong acid dissociates completely in an aqueous solution to furnish the hydrogen ions (H+).…

Q: A 0.75 M solution of a certain weak base has a pH of 11.60. What is the K, for this weak base? O 3.6…

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Q: Calculate the concentration of free Ca2 in a solution of 0.10 M CaY2 at pH 6. K for CaY2 is 4.9x1010…

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Q: Calculate the pH of the following solutions: 1-  0.01 M NaHS 2- 0.005 M NaH PO, 3- 0.005 M NaHPO 4-…

A: Given,  1-  0.01 M NaHS2- 0.005 M NaH2PO43- 0.005 M Na2HPO44- 0.005 M Na3PO4 5-  0.1 M NHCN…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.