Chem101 app.101edu.co Question 19 of 23 Submit What is the pH of a 0.820 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)? 1 4 6 C 7 8 9. +/- x 100

Q: What is the pH of 0.125 M  Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)?  Express your answer to two decimal…

A: Given that 0.125 M Fe(NO3)3 is present. Fe+3 has a Ka value of 3.00×10-3. The equation used to find…

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 0.210 M NANO2? (Ka of HNO2 is 4.5 x 10-4)

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x…

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Q: Calculate the pH of a 0.17 M solution of sodium hydrogen sulfite,

A: Given concentration of NaHSO3= 0.17 M  Ka = 6.0×10-8

Q: What is the pH of a 0.150 M solution of aniline (CeH;NH2, Kb = 4.3 × 10-1º)?

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Q: You have an aliquot of 10 mL of 0.1022 mol/L phosphoric acid.  The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: What is the pH of a 1.75 M solution of KX (Kb of X is 1.22 x 10°) (Please show the final result with…

A: Answer:  9.66 Weak base can't dissociate completely, it's  pOH = 1/2 (PKb - logC)

Q: Calculate the pH of a solution that is 0.0510 M in а. Н3РОД (Ка1 — 7.1 х 10 3). pH = b. НзРОз (Кal =…

A: It's a multiple part question.   Given information, Concentration of the given compounds = 0.0510 M…

Q: Find the pH of a solution containing 0.22 M alanine (NH2CH(CH3)COOH) (pKa1= 2.34, pKa2= 6.87)

A: A sample of alanine is given.Concentration of alanine = 0.22 MpKa1 of alanine = 2.34pKa2 of alanine…

Q: Calculate the pH of the follo 0.39 M NH4CI (рКp fo O a. 2.57 O b.4.83 с. 9.67 O d.4.33 O e. none of…

A: Given, pKb = 4.74  Concentration of Salt(C)= 0.39 M It is salt of weak base -strong acid type salt .…

Q: 12. Sodium Azide (NaN3) is sometimes added to water to kill bacteria. Calculate the pH of a 0.010…

A: Step 1: The chemical equation for the ionization of the azide ion in water isBased on the given…

Q: You have an aliquot of 12 mL of 0.1010 mol/L phosphoric acid.  The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: Calculate the pH, [H2L*], [HL], [L] for each solution of the amino acid proline (Kal = 1.12 x 102…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What is the pH of these solutions? 0.100M sodium acetate CH3CH2O2Na, Kb=5.6x-10 A solution that is…

A: Given solutions are 0.100M sodium acetate CH3CH2O2Na, Kb=5.6x10-10 A solution that is both 0.050M…

Q: You have an aliquot of 11 mL of 0.1093 mol/L phosphoric acid. The ka values for phosphoric acid are…

A: Volume of phosphoric acid = 11 mLMolarity of phosphoric acid sample = 0.1093 mol/LVolume of NaOH…

Q: What is the pH of a 0.223 M LINO2 solution at 25 °C (Ka for HNO2 = 4.0 x 104)? (the answer should be…

A: Given, [LiNO2] = [Salt]=0.223 M Ka of HNO2= 4.0×10-4 pH = ?

Q: What is the pH of an aqueous solution that is 0.011 M CH3COOH (Ka = 1.8 x 10-5) and 0.019 M…

A: An aqueous solution containing weak acid (CH3COOH) and it's conjugate base (CH3COONa) results in the…

Q: What is the pH of 0.0800 M Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)? Express your answer to two decimal…

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Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: What is the pH of a 0.580 M solution of NaCN (Ka of HCN is 4.9 x 1010)?

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Q: Calculate the percent ionization and the pH of the following solution of benzoic acid, HC7H5O2 (Ka =…

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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: 3. What is the pH of a 1.15 M solution of methanoic acid? K = 1.8 x 104

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Q: A solution is prepared at 25 °C that is initially 0.12M in dimethylamine ((CH3), NH), a weak base…

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Q: What is the pH of 0.125 M  Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)?  Express your answer to two decimal…

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Q: Please don't hand riteeg solution

A: The objective of this question is to calculate the pH of a solution of acetic acid (CH3CO2H). The pH…

Q: 0) What is the pH of a solution made by mixing 10.00 mL of 0.25 M acetic acid with 10.00 mL of 0.25…

A: Molarity of acetic acid solution= 0.25 M Volume of acetic acid solution= 10.00 mL Molarity of KOH…

Q: The kw for water is 5.5 x 10-14 at 50oC.  What is the pH of a neutral aqueous solution at 50oC?…

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Q: 9. Calculate the pH of a 0.20 M solution of iodic acid (HIO3 and K₂ = 0.17). [78] 10. Calculate the…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What is the pH of a 0.810 M solution of Ca(NO₂)2 (Ka of HNO₂ is 4.5 x 10-4)?

A: Here first we need to calculate the molarity of NO2- which is conjugate base of HNO2 from given…

Q: I have ammonia (20 M) dissociating in water.  I add 2M ammonium Chloride to the ammonia.  Kb=1.8 x…

A: Answer:- this question is answered by using the simple concept of calculation pH of a solution…

Q: What is the ratio of NH4* to NO₂ in O2-saturated water when the pH is 8.20 and the pE is 4.42?…

A: The question is based on pH of solution.

Q: The pH of 30.0 mL of 0.80 M Benzoic acid (Ka = 5.6 x 10-5) is _____________ (with 3 significant…

A: There are two types of types of acids/bases. Strong acids and strong bases are those acids and bases…

Q: 17. What is the pH of a 0.024 M acetic acid (K₁ = 1.8 x 105) solution at 25 °C? A: 3.18

A: Ostwalt diluation law gives then concentration of H+ ions.

Q: The kw for water is 5.5 x 10-14 at 50oC.  What is the pH of a neutral aqueous solution at 50oC?…

A: Given , kw for water is 5.5 x 10-14 at 50oC.

Q: What is the pH of a 0.650 M solution of C5H;NHB (Kb of CsH;N is 1.7 × 10-º)?

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Q: What would be the pH of a solution prepared by adding 0.130 moles of hydroxide ion to 0.26 moles of…

A: The balanced reaction between acid(HA) and base(BOH) to form salt(BA) and water(H2O) is as follows:…

Q: Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8)  What…

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Q: 1. A chem 101 student dissolves 10.6 g of hydrosulfuric acid (H₂S) in 120 mL of water. Calculate the…

A: Mass of H2S = 10.6 g  Volume of water = 120 mL or  = 0.120 L

Q: NH3 is a weak base (K, = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.