Q: 101. The pH indicator phenol red turns pink or magenta when the pH of the medium becomes more (basic…
A: Note: Since you have posted a question with multiple subparts, we will solve the first three…
Q: 11. What volume of 0.115 M HCl solution is needed to prepare 350.0 mL of a solution of HCl with pH…
A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…
Q: 17. The [H3O+] or [H*] of a solution with pH = 8.7 is what? ([H*)=M] (Use your calculator to find…
A: #17: Given the pH of the solution = 8.7
Q: 7. A chemist mixed 68.5 mL of 0.724 M HNO3 and 95.0mL of 0.0045 M KOH in a reaction vessel. a.…
A:
Q: 13. Which of these statements (to a close approximation) is true of a solution prepared by…
A: In this question, which statement is true ( A, B, C or D ) when NaA dissolving in water. How we can…
Q: 14.7 What is the pH of each solution? a ) 2.2 x 10-2 Μ ΝΟ; b) 1.05 М HI c) 0.011 mol of HCIO4 in…
A: The solutions are
Q: What is the concentration of OH− at 25o C in 0.25 M nitric acid solution?
A:
Q: Calculate the value of H,O* from the given [OH] in each solution and label the solution as acidic or…
A: pH = - log [ H3O+ ] [ H3O+ ] = 10-pH pOH = - log [ OH- ] [ OH- ] = 10-pOH pH +…
Q: A diprotic acid (H₂A) has Kai - 4.55 x 10-7 and K₁2 = 6.07 × 10-¹¹. What is the pH of a 0.463 M H₂A…
A:
Q: A diprotic acid (H₂A) has Kal = 4.28 x 10-7 and K₁2 = 5.45 x 10-¹1. What is the pH of a 0.431 M H₂A…
A: Firstly we find the concentration of H+ ion. Then we find the pH. Shown in step 2.
Q: The [OH-] = 1.3 x 10–6 M for a 0.025 M solution of a weak base. Calculate the value of Kb for this…
A: Consider the given information is as follows; OH- = 1.3×10-6 MConcentration of weak base BOH = 0.025…
Q: What is the pH of a solution that is 0.100 M NH3 and 0.350 M NH4CI? Kb of NH3 = 1.8 x 10-5 9.26 9.80…
A:
Q: 1. A1.0 M solution of a weak base B has a pH of 11.60. What is the valve of Kb for this base? а. 6.3…
A:
Q: For the diprotic weak acid H2A, Kal = 3.9 x 10-6 and K22 = 7.7 x 109 What is the pH of a 0.0400 M…
A: The hydronium ion concentration can be calculated using ICE table as,
Q: (a) Calculate the OH¯ concentration in an aqueous solution at 25°C with an H3O™ concentration of…
A: [H3O+].[OH-] = Kw Kw is the ionic product of water
Q: 6. a) What is the pH of pure water at 35.0 °C? At this temperature Kw = 2.042 x 10-14. b) Based on…
A: (a) The chemical equation for self-ionization of water is: Thus, At 25oC, Kw = 1.0 * 10-14 and…
Q: Sulfurous acid (H, SO,) is a diprotic acid with Kal = 1.39 × 10-2 and K2 = 6.73 x 10–8. Determine…
A: In this question, we will determine the pH of the solution you can see details solution below.
Q: A salt is added to water which has a pH of 7.0. The addition of the salt changed the pH of the…
A: Given that, Initially pH=7.0 After addition if salt, pH changed to 6.2
Q: Indicate which salt in each of the following pairs forms themore acidic (or less basic) 0.010 M…
A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…
Q: What is the pH of a solution when 25 ml, 0.200 M of salicylic acid CeH:(OH)COOH is diluted to 100.0…
A: Given: Concentration of salicylic acid i.e. HA (Assuming it HA as its monoprotic acid) = 0.200 M…
Q: A solution of 0.240 M KOH is used to titrate 10.0 mL of a 0.184 M H3PO4 solution. What volume, in…
A: Since you have posted multiple questions, we are entitled to answer the first only.
Q: 22) The POH of 0.180 M NaCN (basic salt) (Kb of CN¯ = 2.22 x 10°) is: a) 10.9 b) 4.68 c) 3.09 d)…
A: The concentration of basic salt (NaCN) = 0.180 M The equilibrium constant, Kb of CN– = 2.22 × 10–9…
Q: 6. a) What is the pH of pure water at 35.0 °C? At this temperature Kw = 2.042 x 10-14. b) Based on…
A: Water (H2O) molecule is dissociates as, At equilibrium the product of concentrations of H+ and OH-…
Q: What is the pH of a cleaning solution with a [H3O+] = 7.4 x 10-9 M H3O+?
A: Since the pH of any solution is given by pH = -log[H3O+] where [H3O+] = concentration of H3O+
Q: A diprotic acid, H,A, has acid dissociation constants of Ka = 4.88 x 10-4 and K2 = 5.41 x 10-12.…
A: The dissociation of diprotic acid H2A can be written as; H2A (aq)⇔H+(aq) + HA-(aq)…
Q: Calculate the pH of 0.30 M NaOH solution ? Kw = 1.0 x 10-14
A: pH is defined as the concentration of hydronium ion in the solution
Q: How many moles of benzoic acid, a monoprotic acid with K, = 6.4 x 10 5, must be dissolved in 250. mL…
A: Benzoic AcidChemical formula = C6H5COOHAqueous solution benzoic acid has following…
Q: Which of the following statements is TRUE for a solution containing 0.01 M HF(Ka = 6.6 x 10^-4) and…
A: To find: Which among the following statements are true regarding 0.01 M HF(Ka = 6.6 x 10-4) and 0.01…
Q: A solution of 2.5 M weak acid is 1.52% ionized. What is the Ka value of this acid? cof O 32x 104 O…
A:
Q: show ur work(calculation) and answer properly
A: We are given a weak base, it's concentration and percentage ionisation is given. We have to find kb.
Q: What is the pH of a 0.258 M aqueous solution of sodium nitrite, NaNO2 at 25 °C? (Ka for HNO2 =…
A:
Q: A 1.0 M solution of HNO3 was used to neutralize 100.0 ml of 0.20 M Ba(OH)2. b. How many ml of…
A: The dilution formula is as follows, M1V1=M2V2 Where, M1 and M2 are the molarities. V1 and V2 are the…
Q: Which salt produces the most basic solution at a concentration of 0.1M? KF CaC12 NaNO3 NH4CI NaCI Oo…
A:
Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO and 0.49 M in HIO? The Ka for HIO is 2.3…
A:
Q: What is the pH of 500.0 mL of a 0.1 M NaOH solution? O A. 13 О В. 1 ОС. 1.3 O D. 12.7 47L Ansuers to…
A: Given : Concentration of NaOH solution = 0.1 M
Q: Acid Base Neutralization a) What is the pH of a solution of 20 mL of 0.2 M HBr pH =…
A:
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: 1.58 x10-M b) Ca(OH)2 Calculate pH of 0.1 M solution of a weak base with Kb = 1.65 x10-7 %3D P=3.89
A: Weak base is taken as B.An ICE table is constructed to determine the equilibrium concentration of…
Q: A flask of 0.70 M HBrO2(aq) has what pH? (Ka = 1.2 x 10-5) A 2.18 B 2.16 C 3.20 D 2.66 E 1.90
A: Given data contains, Molarity of HbrO2 is 0.70 M. Ka is 1.2 x 10-5.
Q: 11. If 80 ml of a .95M HOCN is reacted with 100 ml of a .80M solution of CSOH, what is the resulting…
A: Whenver an acid and base reacts with each other than they form salt and water and the process is…
Q: B. What is the pH of 0.75 M HC:H3O2 solution? K.= 1.8 x 105 and Kw=1.00 x 10-14 HC:H3O2 + H2O H30 +…
A: Calcuation as shown below
Q: What is the hydronium ion concentration in 0.0200 M HClO? Ka = 2.88 x 10-8
A: In order to calculate the concentration of the hydronium ion we first write down the given data:…
Q: 12. What is the pH of a 2.5 x 10 M hydrobromic acid solution? а. 2.60 b. 11.40 с. 2.30 d. 11.70
A: A 2.5 * 10-3 M HBr solution means the concentration of H+ is 2.5 * 10-3 M. Then the pH of this…
Q: What mass of Ca(OH) is required to neutralize 50.00 mL of 0.180 M HCI?
A: Given information:Volume of HCl = 50.00 mLConcentration of HCl = 0.180 M
Q: 2. If we mix 0.50 mol NaOAc and 0.50 mol HCIO into 1-L solution, the resulting solution should have…
A: Given: Moles of NaOAc mixed = 0.50 mol Moles of HClO mixed = 0.50 mol Volume = 1 L Kb(OAc-) =…
Q: What is the pH of a solution of 0.30 M CH:NH:Cl? Kb for CH:NH2 = 4.4 x 104
A:
Q: What volume of 1.556 mol L solution of LIOH is required to make 5.40 L of a solution with a pH =…
A: Initial Molarity of LiOH ; M1 = 1.556 mol.L-¹ = 1.556 M V1 = volume of 1.556 M of LiOH solution…
Q: 9. (a) What is the pH of () 0.10 М КОН (ад) (ii) 0.15 M HNO3(aq) (iii) The solution resulting from…
A: According to given problem, at first we have to calculate the pH values of a strong base (KOH), a…
Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.28. What is the Kb of this base?
A:
Q: For the diprotic weak acid H₂A, Kal = 2.8 x 10-6 M and K₁2 = 8.9 x 109 M. What is the pH of a 0.0450…
A: Introduction : Diprotic acid are those acids which produces two moles of hydrogen when they are…
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- What volume of 0.120 M NaOH must be added to 100. mL of 0.100 M NaHC2O4 to reach a pH of 4.70?Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
- The pH of a solution of Ba(OH)2 is 10.66 at 25 . What is the hydroxide ion concentration in the solution? If the solution volume is 125 mL, what mass of Ba(OH)2 must have been dissolved?Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 = 8.5 107 N2H5+(aq) + H2O() N2H62+(aq) + OH(aq) Kb2 = 8.9 1016 (a) What is the concentration of OH, N2H5+ and N2H62+ in a 0.010M aqueous solution of hydrazine? (b) What is the pH of the 0.010M solution hydrazine?Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
- You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.Given the acid-base indicators in Question 37, select a suitable indicator for the following titrations. (a) sodium formate (NaCHO2) with HNO3 (b) hypochlorous acid with barium hydroxide (c) nitric acid with HI (d) hydrochloric acid with ammonia
- Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/AA buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?Even though Ca(OH)2 is an inexpensive base, its limited solubility restricts its use. What is the pH of a saturated solution of Ca(OH)2?