Anita added a drop each of diluted acetic acid and diluted hydrochloric acid on ph paper and compared the colors. which of the following is the correct conclusion?

\( \newcommand\) • • • • • • • • • • • • • • • • • Objectives • To set up and show how to use a pH indicator • To determine the pH of common solutions • To understand pH differences of acids and bases • To learn to use a laboratory pH meter • To understand relationship between pH and H+ ion concentration A pH value is a number, usually between 0 and 14, that represents the acidity or basicity of a solution. The “pH” is always written with a lowercase “p” and an uppercase “H”, which stands for “power of hydrogen.” pH values are related to hydrogen ion (\(\ce\)) and checking the pH after each addition. If the pH changes only slightly, the solution is a good buffer. Eventually its buffering capacity will be exhausted, however, and the pH will change dramatically. Materials and Equipment 400-mL beaker, ring stand, wire gauze, Bunsen burner, large test tubes, dropper pipet, stirring rod, wash bottle with distilled water, laboratory pH meter, 0.1 M acetic acid, 0.1 M \(\ce\)), pH paper Part A: Preparing pH indicator and pH standards - INSTRUCTOR DEMO • Tear a few leaves of red cabbage into small pieces and place the leaves into a 500-mL beaker. Add about 500-mL of distilled water to this beaker. Make sure that all of the leaf pieces are completely submerged. • Gently boil the mixture on heating plate until it appears dark purple in color (5-10 min). Turn off the heat and allow to cool (5 min). • Add cabbage indicator solution to pH standard solutions, labeled 1-13. Students will...

Anita added a drop each of diluted acetic acid and diluted hydrochloric acid on pH paper and companis. colors. Which of the following is the correct conclusion? • pH of acetic acid is more than that of hydrochloric acid. • pH of acetic acid is less than that of hydrochloric acid. • Acetic acid dissociates completely in aqueous solution. • Acetic acid is a strong acid Views: 5,257 11 × 2 = 22 1. Explain in which of the following compounds, the chemical bond would have less ionic character : LiCl or KCl. 2 What is activation energy? Establish the relation between rate constant of a reaction and activation energy. 3.. Discuss briefly the structure of CsCl. 4. The osmotic pressure of sugar solution is 2.46 atm at 2 7 ∘ C. Calculate the concentration of the solution. 5. How is molarity of a solution different from molality. 6. Piscuss Raoult's law of relative lowering of vapour pressure. 7. How many moles of Cu will be deposited by passing 24125 coulombs of electric current from CuSO 4 ​ solution? Anita added a drop each of diluted acetic acid and diluted hydrochloric acid on pH paper and companis. colors. Which of the following is the correct conclusion? Updated On Feb 18, 2023 Topic Alcohols, Phenols & Ethers Subject Chemistry Class Class 10 Answer Type Video solution: 1 Upvotes 82 Avg. Video Duration 2 min

\( \newcommand\) • • • • • • • • • • • • • • • • • • • • • • • Learning Objectives Goals: • Understand that parts of an acid-base titration • be able to determine the K aor K bfrom pH data associated with the titration of a weak acid or base • be able to determine the molar mass of a solid monoprotic acid from titration data • be able to calculate K a1and K a2for a polyprotic acid By the end of this lab, students should be able to: • design, develop and performacid base titrations . Prior knowledge: • • Stoichiometry of Acid-Base Titrations in quantitative analysis (s Concurrent Reading & AdditionalResources • pH and pOH ( • pH of Weak Acids and Bases ( • pH of salts ( • buffers ( Safety • Emergency Preparedness • E ye protection is mandatory in this lab, and you should not wear shorts or open toed shoes. The following image shows the damage 4 M sodium hydroxide can cause. By following proper procedures and using proper PPE (Personal Protective Equipment)the risk to damage can be reduced to near zero.There are two primary factors that determine the extent of injury due toexposure to corrosive chemicals like NaOH, the concentration of the chemical and the time of contact (exposure to the chemical). For this reason we do not perform titrations with concentrated acids and bases, but dilute ones. If you ever have an acid or base spill you need to immediately inform your instructor, who will clean it up or instruct you on what to do. If you spill it on your body you should imme...

\( \newcommand\) • • • • • • • • • • • • • • • • • • • Titrations of Strong Acids and Bases Figure \(\PageIndex\). The titration of either a strong acid with a strong base or a strong base with a strong acid produces an S-shaped curve. The curve is somewhat asymmetrical because the steady increase in the volume of the solution during the titration causes the solution to become more dilute. Due to the leveling effect, the shape of the curve for a titration involving a strong acid and a strong base depends on only the concentrations of the acid and base, not their identities. Example \(\PageIndex\) to determine which, if either, is in excess after the neutralization reaction has occurred. If one species is in excess, calculate the amount that remains after the neutralization reaction. • Determine the final volume of the solution. Calculate the concentration of the species in excess and convert this value to pH. Solution A Because 0.100 mol/L is equivalent to 0.100 mmol/mL, the number of millimoles of \(\ce) = 3.5 \nonumber \] This is significantly less than the pH of 7.00 for a neutral solution. Titrations of Weak Acids and Bases In contrast to strong acids and bases, the shape of the titration curve for a weak acid or a weak base depends dramatically on the identity of the acid or the base and the corresponding \(K_a\) or \(K_b\). As we shall see, the pH also changes much more gradually around the equivalence point in the titration of a weak acid or a weak base. As you lear...

Anita added a drop each of diluted acetic acid and diluted hydrochloric acid on pH paper and compared the colors. Which of the following is the correct conclusion? (a) pH of acetic acid is more than that of hydrochloric acid. (b) pH of acetic acid is less than that of hydrochloric acid. (c) Acetic acid dissociates completely in aqueous solution. (d) Acetic acid is a strong acid