Q: What is the strongest base that can exist in liquid ammonia as a solvent?
A: Strongest base that can exist in liquid ammonia as a solvent.
Q: Show how chloric acid (HClO3) can act as an Arrhenius acid when dissolved in water.
A: An Arrhenius acid is that species that will increase the concentration of hydronium ions in the…
Q: 42) What is the [H3O+] concentration of a solution that has a pH = 11.61, 7.156, 0.015
A: pH = -log [H+] = - log [H3O+] pH = - log [H3O+] [H3O+] = 10-pH Use this formula to solve for…
Q: What is the molar concentration of 2.1 % formic acid
A: The question is based on the concept of solutions. molarity is defined as number of moles of solute…
Q: Write a chemical equation showing how each of the following species can behave as indicated when…
A: Acid is a substance which donate hydrogen ions and base is substance which is accept hydrogen ions…
Q: Calculate the H3O+ concentration in a sample of acid rain with a pH of 3.90.
A: pH is defined as the negative logarithm to the base 10 of hydronium ion concentration expressed in…
Q: Complete the autoionization reaction for water. autoionization of water: H2O+H2O↽−−⇀
A: Given :- H2O + H2O → To complete :- above autoionization of water
Q: Based on their molecular structure, pick the stronger acid from each pair of oxyacids. Explain your…
A:
Q: When hydroxylamine acts as a base, which atom accepts the proton?
A: Acid base theory- Acids and bases have their own importance in chemistry. Acids and bases are…
Q: Write a balanced equation showing how the H,PO4 2 ion can be either a Brønsted-Lowry acid or a…
A: When a proton (H+) is donated in any reaction then it is a Bronsted-acid (BA). When a hydrogen ion…
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: Calculate the [H3O+] and pH of a 0.62M NaOH solution.
A: Given, Concentration of NaOH = 0.62M
Q: Write an equation to describe the proton transfer that occurs when HCO3 is added to water and acts…
A: Equation to describe the proton transfer that occurs whenn HCO3- is added to water and act as an…
Q: Which compound forms an acidic solution when dissolved in water?a) NH4Cl b) NaCl c) KNO2 d) Ca(NO3)2
A:
Q: Calculate the H3O+ concentration from each pH: (a) 2.42; (b) 13.39.
A:
Q: Nitric acid reacts with ammonia to yield ammonium nitrate. Write the reaction and identify the acid,…
A: Given here, Nitric acid reacts with ammonia to yield ammonium nitrate and we are asked to write the…
Q: Select the substance that can function as a Lewis acid.
A: A Lewis acid is any substance, such as the H+ ion, that can accept a pair of nonbonding electrons.…
Q: What is the hydroxyl ion concentration of a solution with pH 2.43?
A: pH + pOH =14 pOH = 14-pH pOH =14-2.43 =11.57
Q: Draw beaker drawings for : HBr, a strong acid MgS K2SO4
A: Beaker drawings: In a beaker, the ions of an ionic compound or strong electrolytes will be present…
Q: b Write an equation to describe the proton transfer that occurs when HCO3 is added to water and acts…
A: The answer of following question is given below.
Q: acid , HNO3 , behaves as an acid in water. + H2O(l) =
A: Acid donates protons and base accepts proton.
Q: Given that 65.00 ml of 0.750 M KOH is required to completely neutralize 30.00 ml of an HNO3…
A:
Q: Write a net ionic equation to show how ammonia behaves as a base in water. + H2O
A:
Q: is HCO-3 an acid or base
A: An ion that can react with both acid and base is known as an amphoteric ion.
Q: Which factors affect the relative acidity of an oxyacid?
A: Oxoacids are composed of hydrogen, oxygen, and any other element. In oxoacids, at least one hydrogen…
Q: Calculate the pH of a 0.645 M NH3 solution.NH3 has a ?b=1.8×10−5
A:
Q: Why is the hydronium ion concentration in a solution that is 0.10 M in HCl and 0.10 M in HCOOH…
A: Weak acids: In solution, weak acids do not ionize fully means it ionizes partially in the…
Q: Given the reaction: NH 4 + + C 3H 5O 2 ↔ NH 3 + HC 3H 5O 2, the Bronsted-Lowry base in the reverse…
A: Given :- NH4+ + C3H5O2 ↔ NH3 + HC3H5O2 To identify :- Bronsted-Lowry base in the reverse reaction
Q: Write balanced equations showing how the hydrogen oxalate ion, HC2O4˗, can be both a Bronsted acid…
A: HC2O4˗ is an amphoteric compound. Bronsted-Lowry conjugate acid-base pair: When an acid is dissolved…
Q: For C5 H10NH2™, enter an equation that shows how the cation acts as an acid.
A: According to Bronsted-Lowery acid-base theory, acids are proton donors and bases are proton…
Q: Rank these substances by acidity: 1 = most acidic, 5 = least acidic 4 3.
A:
Q: Write separate equations representing the reaction of H2 PO4−(a) as a base with HBr(b) as an acid…
A: A base is a substance which accepts proton An acid is a substance which donates proton
Q: Write separate equations representing the reaction of HSO3−(a) as an acid with OH−(b) as a base with…
A: HSO3- is amphiprotic. It can act as an acid as well as base.
Q: What are the products of the reaction between nitric acid [HN03(aq)] and sodium hydroxide…
A: The reaction of a strong acid with a strong base gives salt and water. This type of reaction is…
Q: Identify the following species: KClO HHlO4 NH4Cl H2SO4 The choices to pick from for each are as…
A: An acid is a substance which has the tendency to furnish H+ ions in the aqueous solutions. For…
Q: HBrO will act as a Bronsted-Lowry acid or base when reacting
A:
Q: What concentration of NH4NO3 is required to make [OH‐] = 1.0 × 10‐⁵ in a 0.200 M solution of NH3?
A:
Q: Which best defines an acid? A substance that absorbs H in solution A substance that releases OH in…
A:
Q: Write a net ionic equation to show that nitrous acid behaves as a Brønsted-Lowry acid in water. BL…
A: Bronsted–Lowry theory, also called the proton theory of acids and bases, states that any compound…
Q: Give the equations for the hydrolysis of: HCO3 (as a base)
A: A base is defined as a substance which donates its electron pair to an electro-deficient site are…
Q: What is Bronsted acidity? Draw a picture to explain it.How is it measured?
A: Bronsted acidity of any molecule is defined as the tendency of any acid to release H+ ions in the…
Q: Sodium hydroxide is used to clear clogged drains. A solution of NaOH has a pH 1 2 of 9.52 at 25C.…
A: Given, pH of NaOH solution = 9.52 Calculate the pOH = ? Calculate the [H3O+] = ? Calculate the…
Q: How many grams of NahCO3 are required to neutralize 15.0 mL of a solution having a ph of 1.8?
A: NaHCO3 is a base which reacts with acid.Acid gives hydrogen ions in the solution.pH=-log10H+hence,…
Q: Saliva has a pH range of 5.8–7.1. Approximately what is the H3O+ concentration range of saliva?
A: The concentration of the H3O+ ion present in a solution can be related to the pH of the solution as…
Q: write down an equation for the reaction of ammonia solution (NH3) and hydrogen bromide (HBr) and…
A: Bronsted acid :- Species which can donate proton (H+) to other is known as acid Bronsted base :-…
Q: Based on their relative acid strength, is the given comparison correct? HNO3 > HNO2
A: Strength of an acid depends on how many protons are dissociated and form hydrogen ions in…
Q: What is the concentration of H⁺ in 2.0 M acetic acid, HC2H3O2?
A: Given, concentration of acetic acid =2.0 Mwe are asked to find the concentration of H+ in 2.0 M…
Q: Is NH3 an Arrhenius base? Explain.
A: Chemistry related to acid and base was explained by Ostwarld and Arrhenius in molecular way.…
Please briefly explain question no 04
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- A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00 mL portion to a phenolphthalein end point requires 21.25 mL of 0.1385 M HCl. A second 50.00 mL aliquot requires 45.48 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of Na2CO3 in the original solution. (Do not include the unit for molarity. Enter your answer to three significant figures.)What will be the appropriate pH of a buffer prepared by mixing 100 ml of 0.1 M Na2HPO4 and 100 ml of 0.1 M NaH2PO4? (For H3PO4, pKa1 = 2.1; pKa2 = 6.8; pKa3 = 12.5) Ans in 2 significant figuresAn analytical chemist is titrating 230.5 mL of a 0.1500M solution of isopropylamine ((CH3)₂CHNH₂) with a b 0.4100M solution of HNO3. The pK, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 60.1 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
- An analytical chemist is titrating 53.9 mL of a 0.6000 M solution of trimethylamine ((CH,),N) with a 0.7900 M solution of HNO3. The p K, of 3 trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 46.9 mL of the HNO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. olo pH = 0 ? ArEthylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is 0.00298 M ethylamine and 0.00546 M ethylammonium chloride.An analytical chemist is titrating 199.8 mL of a 0.1100M solution of trimethylamine ((CH3), N) with a 0.2200 M solution of HNO3. The pK, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 61.2 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0 X S 图 dh
- A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H₂C6H6O6] = 5.5 X 10-5 M, [HC6HO6¹¹] = 3.5 X 104 M, and K₂ = 8.00 x 10-5 ? everything is based upon the acid dissolving in water: H₂C6H6O6 + H₂O HC6H6O6¹¹ + H3O+1 [ |][ Ka = [ solve for [H3O+¹] then put in the numbers Ka [ [H3O+¹] = [ [H3O+¹] = pH = -log a. H30+1 b. OH-1 h. HCzH3O2 i. C₂H3O₂-¹ = c. H₂C6H6O6 q. 3 r. 0.5000 s. 5.5 X 10-5 x. 5.5 x 10-² dd. 0.7100 ] y. 0.7000 z. 1.60 x 10-5 ee. 1.26 x 10-5 ff. 4.901 ( d. HC6H606¹¹ j. H₂S k. HS-1 t. 3.5 X 10-4 -1 e. HSO3¹¹ 1. S-² X( m. HX f. SO3² n. X-1 g. H₂SO3 o. 1 p. 2 W. 1.11 x 10-8 u. 8.00 x 10-5 v. 1.75 x 10-6 aa. 1.143 x 105 bb. 0.4900 cc. 1.104 x 10-5 gg. 7.93 hh. 4.942 ii. 4.9571. Calculate the pH of buffers that contain the acid and conjugate base in following concentrations: (a) [HPO42-] = 0.33 M ; [PO43-] = 0.52 M (b) [CH3COOH] = 0.40 M ; [CH3COO-] = 0.25 MAn analytical chemist is titrating 159.0 mL of a 0.05700M solution of diethylamine ((C₂H₂)₂NH) with a b 0.2000M solution of HIO3. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 18.4 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = 0
- The normal pH of blood is 7.40 6 0.05 and is controlled in part by the H2CO3/HCO3- buffer system.(a) Assuming that the Ka value for carbonic acid at 25oC applies to blood, what is the [H2CO3]/[HCO3-] ratio in normal blood?(b) In a condition called acidosis, the blood is too acidic. What is the [H2CO3]/[HCO3-] ratio in a patient whose blood pH is 7.20?suppose we drop (10ml of 1 M) of strong base (NaOH) into our buffer. Calculate the PH value for this buffer if the concentration of acetic acid [CH3COOH]=0.09M, and the concentration of [CH3COO-J=0.11M.(P.ka =4.74) снзсоон +он эснзсоо-+ н20 5.21 O 4.22 3.11 O 4.92A 100.0 ml solution containing 0.750 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.239 M KOH. Calculate the pH of the solution after the addition of 54.0 ml of the KOH solution. Maleic acid has pK, values of 1.92 and 6.27. pH = At this pH, calculate the concentration of cach form of maleic acid in the solution at equilibrium. The three forms of malcic acid are abbreviated as H, M, HM", and M", which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. %3D |HM"| = H,M)- please explain and answer each
