chemistry

Sodium thioantimoniate

Sodium thioantimoniate is a chemistry topic covered in the lgStudy science library. This page brings together a partial reference excerpt, illustrations, worked examples, real-world applications and a short study plan, so you can understand Sodium thioantimoniate rather than just read about it. In short: Sodium thioantimoniate or sodium tetrathioantimonate(V) is an inorganic compound with the formula Na3SbS4. The nonahydrate of this chemical, Na3SbS4·9H2O, is known as Schlippe's salt, named after Johann Karl Friedrich von Schlippe (1799–1867).

Key takeaways

Sodium thioantimoniate belongs to chemistry; place it in that map before memorising details.
Learn the definition first, then one example that makes the definition concrete.
Connect Sodium thioantimoniate to a quantity you can measure, compute or draw — that is where exam questions come from.
Reproduce the core statement of Sodium thioantimoniate from memory before moving on to harder problems.

Reference excerpt

Sodium thioantimoniate or sodium tetrathioantimonate(V) is an inorganic compound with the formula Na3SbS4. The nonahydrate of this chemical, Na3SbS4·9H2O, is known as Schlippe's salt, named after Johann Karl Friedrich von Schlippe (1799–1867). These compounds are examples of sulfosalts. They were once of interest as species generated in qualitative inorganic analysis.

Structure

The nonahydrate consists of the tetrahedral tetrathioantimonate(V) anions SbS3−4 and sodium cations Na+, which are hydrated. The Sb-S distance is 2.33 Å. Related salts are known for different cations including ammonium and potassium. The anhydrous salt is a polymer with tetrahedral Na and Sb sites.

Preparation Sodium tetrathioantimonate nonahydrate is prepared by the reaction of "antimony trisulfide", elemental sulfur, and aqueous sulfide source.

3 Na2S + 2 S + Sb2S3 + 18 H2O → 2 Na3SbS4·9H2O The Na2S can be generated in situ by the reaction of sodium hydroxide and S (co-generating sodium sulfate):

Sb2S3 + 8 NaOH + 6 S → 2 Na3SbS4 + Na2SO4 + 4 H2O Charcoal can also be used to reduce the sulfur. The required antimony trisulfide is prepared by treatment of Sb(III) compounds with sulfide sources:

2 SbCl3 + 3 H2S → Sb2S3 + 6 HCl

Reactions The hydrate dissolves in water to give the tetrahedral SbS3−4 ion. The salt gives antimony pentasulfide upon acidification:

2 Na3SbS4 + 6 HCl → Sb2S5 + 6 NaCl + 3 H2S

Notes

References This article incorporates text from a publication now in the public domain: Chisholm, Hugh, ed. (1911). "Schlippe's Salt". Encyclopædia Britannica (11th ed.). Cambridge University Press.

Illustrations

Worked examples

Example 1 — a first encounter with Sodium thioantimoniate

Start with the simplest possible case. Write down what Sodium thioantimoniate claims or describes in one sentence, then invent the smallest concrete situation in which that sentence is true. In chemistry, the smallest case is usually a single object, a single equation or a single measurement. Check that every symbol or term in your sentence has a meaning in that case.

Example 2 — changing one variable

Take the situation from Example 1 and change exactly one quantity: double it, halve it, or set it to zero. Predict what should happen to Sodium thioantimoniate before you calculate. Comparing your prediction with the result is the fastest way to find out whether you understand the idea or only the words.

Example 3 — an exam-style question

Typical questions about Sodium thioantimoniate ask you to (a) state it precisely, (b) apply it to given data, and (c) explain a limitation. Practise writing all three answers in under five minutes; the third part is what separates a full-mark answer from an average one.

Applications of Sodium thioantimoniate

In research: Sodium thioantimoniate appears in chemistry research whenever the underlying quantities have to be modelled precisely. Papers usually cite it as a starting assumption and then explore where it breaks down.
In technology and industry: Engineering practice reuses Sodium thioantimoniate in design rules, simulations and safety margins. Knowing the idea lets you read a specification sheet and understand why the numbers look the way they do.
In the classroom: Sodium thioantimoniate is common in secondary-school and first-year university syllabi. It links to neighbouring topics Antimony(V) compounds, Sodium compounds, Sulfides, so understanding it makes those chapters shorter.
In everyday life: Look for Sodium thioantimoniate outside the textbook — in sport, cooking, traffic, electronics or the sky above you. An example you found yourself is remembered far longer than one you were given.

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How to study Sodium thioantimoniate in 20 minutes

Read the reference excerpt below once, without taking notes.
Close the page and write down what Sodium thioantimoniate means in your own words.
Compare your version with the excerpt and mark what you missed.
Work through the three examples above with pen and paper.
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Frequently asked questions

What is Sodium thioantimoniate in simple terms?

Why does Sodium thioantimoniate matter?

Because it connects several chemistry ideas at once: it gives you a definition you can apply, a quantity you can calculate, and a way to check whether a result is plausible.

How should I study Sodium thioantimoniate?

Read the excerpt, restate it from memory, then work through the examples and applications listed on this page. The five-step study plan above takes about twenty minutes.

What does this page cover?

It gives you a compact reference excerpt plus original lgStudy explanations, examples, applications and study material on Sodium thioantimoniate.