Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its conjugate base is pink in solution. Calculate the

Q: Consider how best to prepare one liter of a buffer solution with pH = 6.52 using one of the weak…

A: Given: The pH of the buffer solution is 6.52. The volume of the buffer solution is 1.00 L.

Q: A 50.0-mL volume of 0.15 mol L¹ HBr is titrated with 0.25 mol L KOH. Calculate the pH after the…

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Q: An unknown solution is red with phenol red and colourless with thymolphthalein. From that…

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Q: A certain indicator, HA, has a K, value of 5.0 x 10-7. The protonated form of the indicator is red…

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Q: Bromcresol green changes color from pH 3.8 to pH 5.4. If the indicator is yellow at pH 3 and blue at…

A: Indicators are substances whose solution changes colour according to the change in pH. These…

Q: Which is the best colored indicator to use in the titration of 0.1 M NH3(aq) with 0.1 M HCl (aq)?…

A: Which one of the correct

Q: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Moles of base taken =Molarity of base×Volume of base=0.0200 mol/L×50.00×10-3L=0.001 mol

Q: If NH4OH (aqueous ammonia, Kp = 1.8 x 10-5) is titrated with HCI, the pH at the equivalence %3D…

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Q: 2 liters of 0.2 M NH4Cl solution 11.4 liters of NH3 solution measured under normal conditions.…

A: We will use formula of pH of salt

Q: Bromthymol blue has a Ka value of 1.0 \times 10-7, is yellow in its HIn form and blue in its In -…

A: To find the pH at which the indicator color change will first be visible, we can think about the…

Q: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Given: Weak base = 0.0200 M Volume of weak base = 50.0 mL Concentration of base = 0.0150 M pKb of…

Q: When an acid solution is titrated with a base, an indicator (HIn) changes from yellow to blue (In).…

A: Answer:An indicator is a chemical substance that indicates about the completion of titration by…

Q: The base dissociation constant for ammonia is 1.8x10-5. If you carry ouit a titration in which you…

A: In the given question we have to calculate the pH of the solution at equivalence point. First of…

Q: Which of the given statements are CORRECT for an indicator that ionizes as shown below (Ka=1.0 x…

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Q: In a system where a weak acid is an analyte, a strong base is a titrant, what is the milestone pH…

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Q: Phosphoric acid is a triprotic acid with the Ka values of 7.25 10-3, 6.31 10-8 and 3.98 10-13…

A: Millimoles of H3PO4 taken   =Molar concentration of acid×Volume of acid=0.1000 M×25 mL=2.5 mmol

Q: The indicator meta-cresol purple is an acid with a Ka of 3.1 ✕ 10−2. In a 2.2 ✕ 10−4 M solution, it…

A: The given sample is meta-cresol purple.Acid dissociation, Ka, of meta-cresol purple =…

Q: A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak…

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Q: Consider an indicator that ionized as shown below for which Ka = 1.0 × 10−4           HIn ⇆ H+ +…

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Q: Pyrazolium Chloride is a weak acid (C3H4N2HCl; Ka=1.4x10-3). How many grams of Pyrazole (conjugate…

A: Given: Ka of C3H4N2HCl = 1.4 X 10-3  Concentration of C3H4N2HCl = 0.3 M And pH of buffer solution =…

Q: Reaction HA(aq) + H20(1) H;O°(aq) + A (aq) Initial conc. / M: 0.0900 Change in conc. at equilibrium…

A: pH  - It is known as the negative logarithm of the hydronium ion concentration of a solution. Ka -…

Q: Phenolphthalein works in the range pH 8 to 12.5 and turns pink in that range. What will occur if…

A: The indicators are chemical compounds that show changes in color at a definite change in pH. Hence,…

Q: solution of 0.0100 M NaOH. The graph obtained from said process is shown below, also a portion of…

A: Weak acid are the acids that do not undergo ionization completely rather maintain equilibrium…

Q: A certain indicator(Hln) has a Ka value of 1.0 x 10^-7.  The protonated form of the indicators is…

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Q: Calculate the concentrations of all species present, the pH and the percent dissociation of HCN (Ka…

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Q: How much (in grams) Na2HPO4 must be added to 100 mL 1.0 M NaH2PO4 solution to prepare a buffer…

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Q: Bromthymol blue has a Ka value of 1.0 \times 10-7, is yellow in its HIn form and blue in its In…

A: To find the pH at which the indicator color change will first be visible, we can think about the…

Q: MOPS is a weak acid that ionizes according the the reversibile chemical equaiton HMOPS 2 MOPS" + H*.…

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Q: Ka

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Q: Given the following hydrolysis constants, which of the salts has the weakest parent ACID? K₂ or K,…

A: given-hydrolysis constants of given salts.SALTK2 OR K for…

Q: Noting that the ratio of weak conjugate base(the anion of the acid) to weak acid in a titration can…

A: Answer: A buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Consider the following information about sulfurous acid, a diprotic acid (H-SO3). H2SO3 = HSO,+H…

A: The titration curve given is, And the titration of Na2SO3 with HCl is given.

Q: An acid-base indicator is usually a weak acid with a characteristic color in the protonated and…

A: Acid-base indicators are commonly used in chemistry to determine the pH of a solution. These…

Q: In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of…

A: In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of…

Q: A certain indicator, HA, has a K value of 0.00025. The protonated form of the indicator is blue and…

A: • The values provided in the question are:-  i) Ka value of a certain indicator HA = 0.00025    •…

Q: analytical chemistry. Given the following titration curve, what is the suitable indicator for this…

A: The above question is based on analytical chemistry . We have to discuss about the roll about the…

Q: Consider how best to prepare one liter of a buffer solution with pH = 6.52 using one of the weak…

A:

Q: A 50.0 ml aliquot of a 0.0010OM solution of acetic acid (K = 1.8 x 10-5) is titrated with 0.00993M…

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Q: Compare conductivity titration to pH-metric titration. Do both methods yield the same equivalence…

A: Answer: Conductivity titration and pH-metric titration are two different methods of determining the…

Q: Which indicator is more suitable for titration of 0.1000 M NH3 with 0.1000 M HCI: methyl orange (pT…

A: In a chemical laboratory, titration is a common analytical technique used to determine the…

Q: Bromthymol blue has a Ka value of 1.0 \times 10-7, is yellow in its HIn form and blue in its In…

A: The objective of the question is to determine the pH at which the color change of Bromthymol blue…

Q: The following table shows the values of ionization constants Kb Formula Ka HC2H302 1.8x10-5 HCIO2…

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Q: HC2H3O2 (aq) + H2O (l) C2H3O2- (aq) + H3O+ (aq) Ka=1.8*10^-5 Calculate the pH of an acetic acid/…

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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.