How do you explain the pattern/trend in the distance between the anion of an acid and H3O+? The acid strength is HCl > HNO3 > HF > HOCl, but I don't understand why the lengths vary like this. Or does it have to do with electronegativity? If it does have to do with electronegativity, why doesn't HF have the shortest length? Or is it because OCl- is more elctronegatvie than F-? Also, does an acid's strength decrease/increase with increasing electronegativity of its conjugate base? When looking at the trend, HI is stronger than HBr, which is stronger than  HCl. However, HClO4 is stronger than all of these acids, which I don't understand why.

Q: Cu2+, Cu2* (ag) + 6 H2O, → Cu(H2O)6* (aq) 2+ (ад)

A: Cu2+ (aq) + 6H2O(l) --> Cu(H2O)62+(aq)

Q: pH

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH of the solution resulting from the addition of 20.0 mL of 0.100 M NAOH to 55.0 mL…

A:

Q: Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an…

A: The solution is as follows:

Q: What is the concentration of a weak acid if its Ka = 3.7 x 10-7 and its pOH = 11.62?

A:

Q: 1. Identify acid or base, give its conjugate form. A) HCO, в) он C) H;SO. D) H:PO.

A:

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 x 10 3, Ka2 = 6.2 x 108,…

A: Dissociation constant are based on ion of H3PO3 .

Q: 6. Calculate the pH of each of the following solutions: a. 2.8x10-4 M Ba(OH)2 b. 5.2x10-4 M HNO3

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pH of a 0.82 M HClO, hypochlorous acid solution, which has a Ka of 3.2 × 10–8 at 25°C?

A:

Q: (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.084 M aqueous…

A:

Q: (b) What will happen if acetic acid (HC2H3O2) is added to water? O An equilibrium will form between…

A:

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: Phosphoric acid , H 3 PO 4 (aq) , is a triprotic acid , meaning that one molecule of the acid has…

A:

Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: Calculate [H3O+][H3O+] given [OH−][OH−] in each aqueous solution. [OH−] = 4.2×10−12 M [OH−] =…

A:

Q: The [OH] in a 0.20M solution of NH4OH is: (Kb for NH4OH = 1.8 x 10-5) 3.6 x 10-6 M O 1.8 x 10-5 M…

A: Given: Initial concentration of NH4OH=0.20 M Kb of NH4OH = 1.8×10-5 Let x be the dissociated amount…

Q: H. 5.7 x 10 -10 1.5 x 10-11 || H 7.9 x 10-12 Br H. В (ад) + H2О(1) нв" (aq) + Он (ад) [HB"][OH [B]…

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

Q: Write the dissociation equations for the following that emphasize their behavior asArrhenius…

A: The dissociation equation for the given acids has to be written.

Q: Which of the following Lewis base has the highest proton affinity in the ga phase? PME3 PF3 PCI3

A: There are many trends in inorganic chemistry. These trends are atomic size, reactivity, metallic…

Q: From what acid and what base are these salts below made from? a. Ca(NO3)2 b. NH4Br c. BaCl2

A:

Q: What mass of NaOH(s) must be added to 1.0 L of 0.045 M NH3 to ensure that the percent ionization of…

A: The reaction happening is as follow:                           NH3 + H2O ----> NH4OH…

Q: Explain what happens to the ratio of the two common forms of free residua! chlorine as the pH of…

A: Hypochlorous acid, HOCl(aq) is a weak acid with Ka = 2.5*10-8  Hypochlorite, ClO-(aq) is a conjugate…

Q: What is the percent dissociation of 0.20 M iodic acid? (The Ka value for iodic acid, HIO3, is 1.7 x…

A: The percent dissociation indicates the relation between concentration of ionized hydrogen ions and…

Q: What are the pH and pOH values of a 0.5454 M aqueous LiOH solution?   pH= 0.699, pOH=13.30…

A: The correct answer is given below

Q: Calculate the pH of a 0.100M solution of the weak base NH3. Kb of NH3 1.8×10. %3D 3)

A:

Q: An environmental concern involves the destructive effects of acid rainfall ever had a pH of 2.4,…

A:

Q: Match the description with the corresponding example: a. HF b. NH3 1. A charged, amphoteric molecule…

A: Answer  Match the description with the corresponding examples…

Q: Phosphoric acid, H3PO4(aq),H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has…

A:

Q: Which of the following solutions, tested by Tania, is a base? Explain the reason why. ELECTRICAL…

A: Acid :-  Acid is a substance which provides excess of H+ ions when it is dissolved in water. Base :-…

Q: Determine the pH of solution if 0.085g of acetylsalicylic acid, HC,H,O4, (Ka = 3.0 x 10) is…

A: Acetyl salicyclic acid ionizes in water as HC9H7O4 + H2O ---->  H3O+ C9H7O4-  (Ka = 3.0 x 10-5)…

Q: Methylammonium halides, like CH3NH3CI (67.52 g.mol), are white or light colored powders used…

A: CH3NH3Cl is salt of a weak base CH3NH2 and strong acid HCl. Therefore, the hydrolysis reaction of…

Q: Which correctly shows the ionization of H2CrO4 in water?

A: The acid given is H2CrO4.

Q: Calculate the theoretical pH of 10 mM NaOH using the data below: • NaOH is a strong base,…

A: We know that, pH is the negative logarithm of hydrogen ion concentration, i.e.…

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: What is the pH of a solution with a hydrogen concentration of 2.3x10-SM? pH pH 2 2 2 3 3 3 5 5 6 6 6…

A:

Q: In a 2.31 M HCOOH aqueous solution, determine the percentage of ionised HCOOH molecules. Ka 1.8 x…

A: Given,  Molar concentration of HCOOH = [HCOOH] = 2.31 M  Acid dissociation constant of HCOOH = Ka =…

Q: a 0.55 M solution of a monobasic compound B has a pH of 11.32, what is the Kb value of the base B

A:

Q: 1. Calculate the H3O* and OH concentrations according to the given ph values. Solution pH [H,O']…

A: Since, pH = - log[H3O+]  => [H3O+] = 10-pH  Since, Kw = [H3O+][OH-]  => [OH-] = Kw/[H3O+] =…

Q: Acid Ka HC3HSO3 1.4 x 104 HOCN 3.5 x 104

A: Given acids,      Lactic acid - HC3H5O3      Cyanic acid - HOCN

Q: The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47. The pH of a 0.300 M solution of…

A: Given: The amount of malonic acid dissolved in 0.250 L is 19.5 g. The pH of malonic acid and 0.300 M…

Q: Drinking water is often disinfected with Cl₂, which hy-drolyzes to form HClO, a weak acid but…

A:

Q: On dissolving 7.258 gm of HCN (Ka=7.2x10 1) in water, the solution become 100 ml so the degree of…

A: HCN is a Weak acid the degree of dissociation of a weak acid or base or an electrolyte was explained…

Q: What mass of NaOH(s) must be added to 1.0 L of 0.072 M NH3 to ensure that the percent ionization of…

A: Given,  Concentration of NH3, [NH3] = 0.072 M

Q: The following two reactions involve proton transfer. In each reaction, identify the acid and the…

A: Acids are substances which have the ability to donate protons and bases are substances which have…

Q: 9. Based on formulas alone, classify each of the following oxoacids as strong or weak. a) H,PO4 b)…

A:

Q: Determine the pH of the solution resulting from mixing a solution of 154 mL of HNO2 (Ka = 5.62e –…

A:

Q: True or false ___________1. The acidity of the solution is higher with higher pH. ___________2. pH…

A: In the given question we have to do True or false of the following question.  1.  False ,  because…

Q: Determine the pOH of a 0.461 M C,H5 COOH solution if the Ka of the acid is 6.5 X 10-5 5.48 O 11.74…

A: We will first write dissociation equation of acid, then calculate H+ concentration to find pH and…

Q: Calculate the pH of a 6.71 x102 M NaOH solution 1.17O 2.17O 6.710 12.83O

A:

Q: Calculate the pH of water containing 0.05 M NaCl at 25°C. Given: YH = 0.86 and %3D YOH- = 0.81. O…

A:

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.