One of the factors that can affect the pH of a buffered solution is the molar ratio of the conjugate base and weak acid. Which of the following statement is correct?     "If the concentration of the conjugate base is higher than the weak acid, the pH will be less than the pKa."     "If the concentration of the conjugate base is less than the weak acid, the pH will be less than the pKa."     "If the concentration of the conjugate base is higher than the weak acid, the net change of the pH is going to the acidic side (lower pH)"     "If the concentration of the conjugate base is less than the weak acid, the net change of the pH is going to the basic side (higher pH)"

Q: Calculate the pH of a blood plasma sample with a total CO, concentration of 25.7 mM and bicarbonate…

A: Given,The total concentration of CO2 is 25.7 mM.The concentration of bicarbonate is 24.4 mM.The pKa…

Q: To what pH should a solution that is 0.072 M each in Ca2+ and Cd2+ lons be adjusted in order to best…

A: The concentration of each of the Cd2+ and Ca2+ ions in the solution is given to be 0.072 M. The Ksp…

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: The compounds given are KCl, Ca(OH)2 and PbF2.

Q: What is the hydronium ion concentration and pH of a 0.20 M solution of hypochlorous acid, Ka = 3.5 x…

A: Since you have posted multiple questions with multiple sub parts,we will provide the solution only…

Q: If the concentration of Mg2+ in the solution were 0.038 M. what minimum [OH-] triggers precipitation…

A: Given :  Concentration of Mg+2 = 0.038 M  Ksp of Mg(OH)2 = 2.06 x 10-13

Q: The K, for acetic acid (CH,COOH) is 1.737 x 10-. What is the pK for this acid? pKa = Use the…

A: 1)          Ka(CH3COOH) = 1.737 x 10-5          pKa = -logKa = -log(1.737 x 10-5)          pKa =…

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: To determine the effects of pH on the solubility of these compounds and identify at which pH the…

Q: What is the equilibrium concentration of chloroacetic acid, HC₂H₂O₂Cl, in a solution prepared by…

A: Given: Moles of HC2H2O2Cl = 0.0271 mol Volume of water = 1.50 L Ka of HC2H2O2Cl = 1.4×10-3

Q: Calculate the pH of a saturated solution of lead hydroxide. See the Solubility Product Constant…

A:

Q: Each of the insoluble salts below are put into 0.10 M hydroiodic acid solution. Do you expect their…

A: 1. **Nickel(II) sulfide (NiS)**:  - NiS is slightly soluble in water. Hydroiodic acid adds a…

Q: nate (Na2CO3)corresponds to the following values: 0.53 M.   (Ka for HCO3− is 5.6 ×10−11.)  Report…

A: Ka = 5.6×10-11 pKa = -log(Ka)   = -log(5.6×10-11) = 10.25 1) As it is Acidic buffer,  pH = pKa +…

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: Solubility of a compound changes with PH, if any constituent ion of the compound reacts with Proton…

Q: The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20.  Suppose a chemist mixed 33.23 mg…

A: 3Mg2+ + 2 AsO43-  ------> [Mg3(AsO4)2] Ksp = 2.00 X 10-20 Mg2+(aq)  = 33.23 mg =  33.23  * 10-3 g…

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: 1) NaBrSince sodium bromide is a salt of strong base (NaOH) and strong acid (HBr), it is a neutral…

Q: We dissolve 3.54 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. We…

A: Any acid's strength always gets estimated by its dissociation constant which is symbolized as "Ka".…

Q: You take 10.00 grams of pure acetic acid add top it up to 1.00 liter of solution

A: Note: Since we only answer upto 3 sub parts we will answer the first 3.Please resubmit the question…

Q: A student determine the k a of an acid to be 5.8722 x 10 -4. What is the pK a?     4.0532…

A: Given, ka of an acid = 5.8722 x 10 -4 pKa = ?

Q: In an experiment, Sadhvi and her lab partner, Nandini, make a buffer containing hydrazoic acid, HN3,…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: Taking into account the effect of activity, calculate the pH of each of the following: 1. 0.10 M…

A: Since you have asked a question with multiple subparts we will answer the first three subparts for…

Q: If  solid CaCl2  is added to a saturated solution of Ca(OH)2 which of the following is correct.…

A: When CaCl2 added to the saturated solution of Ca(OH)2 ,  the concentration of OH- ions decreases due…

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-³, Ka2 = 6.2 x 10-8, and K₁3 = 4.8 x 10-¹3). To…

A:

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A:

Q: A buffer is formed by adding 1.0 mol of trimethylamine, (CH3)3N, and 1.0 mol of trimethylammonium,…

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

Q: (d) Is the groundwater sample described in part (a) at equilibrium with respect to transformations…

A: (d) Water proceeds towards equilibrium here refers in terms of achieving an equilibrium between the…

Q: Strong base is dissolved in 685 mL of 0.400 M weak acid (Ka = 4.21 × 10-³) to make a buffer with a…

A:

Q: In an experiment, the following reagent solutions were mixed to reach chemical equilibrium.  0.2…

A: The objective of the question is to find the initial concentration of SCN- in the reaction mixture.…

Q: Initial (M) Change (M) Equilibrium (M) Determine the pH of a buffer solution by constructing an ICE…

A: Amount of HC7H5O2 = 21.5 gAmount of NaC7H5O2 = 37.7 gVolume of the solution = 200 mLKa of HC7H5O2 =

Q: The Ksp value for calcium sulfate [CaSO4] is 2.40 X 10-5 and a professor made 1825 mL of a CaSO4(2g)…

A:

Q: Solution A: Solution B: Solution C: Solution D: 0.565 M HOCI 0.376 M HC1O4 0.817 M HCO₂H 0.789 M…

A: The pKa of the buffer solution is given by the Henderson-Hasselbalch equation, pKa = pH -…

Q: An analytical chemist is titrating 69.7 mL of a 0.2500M solution of nitrous acid (HNO₂) with a…

A: The objective of this question is to calculate the pH of the acid solution after a certain volume of…

Q: A buffer solution contains a weak acid, HA, and its conjugate base, A. The buffer solution has a pH…

A: Given: The pH of the buffer solution of the weak acid, HA = 5.56 The pKa of HA = 5.00 We have to…

Q: You made a pH 9.0 buffer solution at 25° C by mixing NaOH and histidine (HisH) to give a solution…

A: The buffer considered has pH = 9.00Constituents of the buffer: NaOH and HistidineTotal concentration…

Q: Write the Ksp expression for the sparingly soluble compound iron(III) sulfide, Fe2 S3. (If either…

A: Since, In case of pure liquid and solid is not included in Ksp expression. Because it does not…

Q: A student titrates a weak acid and draws the titration curve. Suppose s/he forgets to subtract off…

A:

Q: In this lab, we will experimentally determine the titration curve for the titration of a weak acid…

A:

Q: You are asked to make a buffer of pH 3.4 and given the above acids. Of these acids, which would…

A: A buffer solution is a mixture of a weak acid and its conjugate base or weak base with its conjugate…

Q: A buffer solution consists of 0,25 mol∙dm–3 acetic acid (HC2H3O2; Ka= 1,8 x 10–5) and 0,35 mol∙dm–3…

A:

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.